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Chemistry Midterm (chapters 2-4,6-10)

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Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 18) water

Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 10) He, H, I

18) Which one of the following elements forms two or more ions with different ionic charges? A)K B)F C) Ca D) O E) Fe

Answer: 25) The bond between Li and F is polar covalent.

False

Match the correct name of the polyatomic ions with the formulas given. A) hydroxide B) hydrogen carbonate C) hydrogen sulfate D) nitrite E) phosphite F) sulfite G) phosphate H) carbonate I) hydrogen sulfite J) nitrate K) oxide L) sulfate M) carbonite 10) PO43-

Match the correct name of the polyatomic ions with the formulas given. A) hydroxide B) hydrogen carbonate C) hydrogen sulfate D) nitrite E) phospbite F) sulfite G) phosphate H) carbonate I) hydrogen sulfite J) nitrate K) oxide L) sulfate M) carbonite 7) CO32-

Water vapor is a gas.

True

15) What is the total pressure (in atm) of a gas mixture, which has CH4 600. torr and He 450. mmHg?

1.38 atm

temperature of 50. °F is equivalent to —°C.

10 °C

9) A 12-g sample of cooking oil, which is a fat, contains— kcal.

108 kcal

6) A gas has a volume of 12.0 L when the pressure is 840. torr. When the pressure changes to 600 torr, what is the new volume, if there is no change in temperature or amount of gas?

16.8 L

16) The total pressure of a mixture of CO2 and O2 is 780 mmHg. If the pressure of the CO2 is 560. torr, what is the pressure of O2?

220. mmHg

temperature of 20°C is equivalent to —-K.

293 K

14) If 450. mL of 6.0 M KBr solution is diluted to 900. mL, the concentration of the KBr solution is —-M.

3.0 M KBr

43) The correct symbol for the isotope of potassium with 22 neutrons is A) 41/19 K B) 19/41 K C)37/15 P D) 15/37 P E) 22/19 K

44) A solution with the same osmotic pressure as the blood is A) isotonic to the blood B) hypotonic to the blood C) hypertonic to the blood D) nontonie to the blood E) molar to the blood

10) An equivalent is A) the amount of ion that has al+ charge B) the amount of ion that has a l- charge C) the amount of ion that carries 1 mole of electrical charge D) 1 mole of any ion E) I mole of an ionie compound

13) A solution contains 43 mEg/L of of Ca- and 11 mEg/L of HPO2. If the only cation in the solution is Na*,what is the Narconcentration in mEg/L? A) 43 mEg/L B) 11 mEgL C) 54 mEg/L D) 32 mEg/L E) 2.0 mEg/L

14) The gas with an initial volume of 24.0 L at a pressure of 565 torg is compressed until the volume is 16.0 L. What is the final pressure of the gas, assuming the temperature does not change? A) 377 torr B) 760 torr C) 848 torr D) 500. torrE) 465 trr

19) In which of the following would the particles move most rapidly? A) ice at -20 °C B) water at 20 °C C) steam at 110 °C D) boiling water E) ice at 0 °C

31) At STP, temperature and pressure have the values of A) OK and I atu B) 273 K and 1 mmig C) 273 K and 760 mmHg D)OK and 760 mmHg E) 760 K and 273 atm

31) What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH? A) 3.0 L B) 0.50 L C) 2.0 L D) 4.5 L E) 0.22 L

41) Which of the following is not a potential use for a hyperbarie chamber? A) treatment for burns and infections B) counteracting carbon monoxide poisoning C) increasing the rate at which a broken bone heals D) treating a diver with the bends E) treating some cancers

43) At STP, what is the volume of 4.50 moles of nitrogen gas? A) 167 L B) 3420 L C) 101 L D) 60.7 L E) 1230 L

43) Which of the following compounds contains an ionic bond? A) NH) B) H30 C) CaO D) H2 E) CH4

44) What is the mass of 53 mL of ethanol, which has a density of 0.79 g/ml? A) 67.1 g B) 41.9 g C) 42 g D) 67 g E) 53 g

46) At STP, what is the mass 13.O L of methane, CH? A) 0.580 g B) 16.0 g C) 931 g D) 27.6 g E) 22.4 g

46) How many calories are required to increase the temperature of 13 g of ethanol from 11 °C to 23 °C? The specific heat of ethanol is 0.59 cal/g °C. A) 83 cal B) 0.63 cal C) 92 cal D) 0.54 cal E) 170 cal

5) In the kinetic molecular theory of gas behavior, particles of a gas tend to move —-and collisions between them are —-A) rapidly, rare B) slowly, rare C) rapidly, elastic D) slowly, elastic E) slowly, unusual

55) A burn from steam at 100 °C is expected to be more severe than a bum from boiling water at 100 °C because A) the steam is hotter than the boiling water B) there is more steam than water C) the steam will give off a large amount of heat as it condenses D) you are more likely to come into contact with the steam than with the boiling water E) All of these answers are correct.

55) The number of electron energy levels in a magnesium atom is A) I B) 2 C) 3 D) 4 E) 5

57) The heat of fusion for water is 80. cal/g. How many calories of heat are needed to melt a 35 g ice cube that has a temperature of 0 °C? A) 2300 cal B) 1600 cal C) 2800 cal D) 540 cal E) 0 cal

59) How many valence electrons are in the electron-dot symbols for the elements in group 3A (13)? A) 1 B) 2 C) 3 D) 4 E) 6

6) What is the ionic charge of an ion with 13 protons and 10 electrons? A) 1+ B) 2+ C) 3+ D) 2- E) 3-

64) The atomic size of atoms A) increases going across a period B) decreases going down within a group C) increases going down within a group D) does not change going down within a group E) none of the above

67) The metallic character of elements A) increases going across a period B) decreases going down within a group C) increases going down within a group D) does not change going down within a group E) none of the above

8) Elements in group 2A (2)of the periodic table form ions with a charge of A) 1+ В) 1- C) 2+ D) 3+ E) 0

8) Water is a polar solvent and hexane (CoH1) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute in the given solvent? A) mineral oil, soluble in water B) Cac2, soluble in hexane C) NaHCO, soluble in water D) CC4, soluble in water E) octane, soluble in water

9) The ion of aluminum is A) Al+ B) A12+ C) A13+ D) A13- E) A12-

A balloon is filled with helium gar. For the following question(s), select the letter of the balloon diagram that corresponds to the given change in conditions 15) The balloon is put into a chamber where the pressure is less than the utmospherie pressure. A) A B) B C)C D) A and B E) B and C

Match the chemical name with the correct formula. A) Mg(HSO4)2 B) MgS04 C) MgS D) Mg(HSO32 E) MgS03 17) magnesium sulfide

Match the statel) of matter with eack of the following descriptions of a substance. A) liquid B) solid + liquid C) gas D) liquid + gas E) solid 2) Great distances exist between the particles.

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 19) 1 mL=. cm3

Match the type of mixture with the appropriate characteristics. A) solution B) colloid C) suspension 14) a mixture whose particles settle on standing

Match the type of mixture with the appropriate characteristics. A) solution B) colloid C) suspension 17) a mixture whose particles can be separated by filters

Select the correct symbol for the element named. 8) silver A)S B) Si C) Ag D) Au E) AG

Write the symbol from the element name. 6) The symbol for silver is

1) The O-H bond in water is polar because A) it is an ionic bond B) oxygen is much more electronegative than hydrogen C) oxygen occupies more space than hydrogen D) hydrogen is much more electronegative than oxygen E) it is a hydrogen bond

1) Which of the following is not part of the kinetic theory of gases? A) A gas is composed of very small particles. B) There is very little empty space in a gas. C) Gas particles move rapidly. D) Gas particles do not attract or repel one another. E) Gas particles move faster when the temperature increases,

10) How many electrons will chlorine gain or lose when it forms an ion? A) lose 1 B) gain 1 C) lose 7 D) gain 2 E) lose 3

11) What elements are in hydroxyapatite, Cas(PO4)sOH, a major compound in human bones and teeth? A) carbon, potassium, oxygen, hydrogen B) calcium, phosphorous, oxygen, hydrogen C) carbon, phosphorous, oxygen, helium D) calcium, phosphorous, oxygen, helium E) carbon, potassium, oxygen, helium

12) The volume of a gas with a pressure of 1.2 atm increases from 1.0 L to 4.0 L. What is the final pressure of the gas, assuming constant temperature? A) 12 atm B) 0.30 atm C) 33 atm D) 4.8 atm E) 1.0 atm

12) Which of the following is a physical change? A) baking a cake B) solid dry ice changing to a gas C) fermenting grapes to produce wine D) digesting a meal E) a tomato ripening

14) Which of the following is a physical change? A) iron rusts B) fce melts C) sugar caramelizes D) food digests E) natural gas burns

17) A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 C What was its new volume? A) 4.84 L B) 5.17 L C) 7.00 L D) 3.57 L E) 4380 L

18) According to Henry's law, the solubility of a gas in a liquid B) increases as the gas pressure above the liquid increases A) decreases as the gas pressure above the liquid increases C) remains the same as the temperature increases D) depends on the liquid polarity E) depends on the liquid density

18) The correct answer for the addition of 7.5 g+ 2.26 g + 1.311g+2 g is A) 13.071 g B) 13 g C) 13.0 g D) 10 g E) 13.1 g

18) Which one of the following properties describes a liquid? A) has its own shape B) particles are close together and move randomly C) particles move very rapidly D) fills the entire volume of the container E) There is essentially no interaction between the particles.

2) According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because A) a gas is composed of very small particles B) the particles of a gas are very far apart C) gas particles move rapidly D) gas particles do not attract or repel one another E) gas particles move faster when the temperature increases

20) If the temperature is 20. °C, what is the corresponding temperature on the Fahrenheit scale? A) -22 °F B) 68 °F C) 43 °F D) 239 °F E) 94 °F

20) The name of the Cut ion is A) copper(II) B) copper(I) C) copper(III) D) сорper E) cuprum

21) A temperature of 125 °C is the same as A) -148 K B) 398 K C) 257 K D) 530. K E) 273 K

21) The elements sodium, magnesium, and silicon A) are isotopes of cach other B) are in the same period of elements C) have the same number of neutrons D) are in the same group E) have the same mass number Answer:

21) What is the metric relationship between grams and micrograms? A) 1 g- 100 ug B) I g=1 000 000 ug C) 1 g=0.000 001 ug D) 1g= 1000 ug E) Ig-0.001 ug

22) The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure in the container is kept constant? A) 210 ml. B) 1170 ml. C) 0.00950 mL D) 0.00474 mlL E) 110 ml.

22) What is the concentration, mass/volume percent (m/v), of a solution prepared from 50. g NaCl and 2.5 L of water? A) 5.0% (m/v) B) 2.0% (m/v) C) 0.020% (m/v) D) 0.050% (m/v) E) 20.% (m/v)

22) Which element would have physical and chemical properties similar to chlorine? A) Ar B) Br C)S D) O E) P

23) In Gay-Lussac's law, the pressure of a gas incereases due to an increase in temperature because A) the molecules strike the walls of the container less often B) the molecules strike the walls of the container more often C) the molecules get bigger D) there is a decrease in the volume of the container E) there is an increase in the number of gas particles

27) An example of kinetic energy is A) a coiled spring B) running water C) a tree D) natural gas E) food

27) The name of the HSO4 ion is A) sulfate B) hydrogen sulfate C) sulfite D) hydrogen sulfite E) sulfide

29) A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atn and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atu and the temperature is 27 C? A) S80 ml B) 630 ml. C) 100 ml. D) 110 ml. E) 1100 ml.

29) Which of the following is an example of potential energy? A) chewing food B) water stored in a reservoir C) burning wood D) a fan blade turning E) riding an exercise bike

34) The mass number of an atom can be calculated from A) the number of electrons B) the number of protons plus neutrons C) the number of protons D) the number of electrons plus protons E) the number of neutrons

34) What is the molarity of a KCI solution made by diluting 75.0 ml of a 0.200 M solution to a final volume of 100. mL? A) 0.267 M B) 0.150 M C) 0.200 M D) 6.67 M E) 0.100 M

36) At STP conditions, 11 g of SO2 have a volume of A) 250 L. B) 3.8 L C) 22 L D) 0.0076 L E) 130 L

38) A cheeseburger from a fast food restaurant contains 19 g of fat, 20 g of carbohydrate, and 28 g of protein. How many kcal of energy does the cheeseburger contain? (The caloric values are: 4 kcal/g for carbohydrate, 9 kcal/g for fat, and 4 kcal/g for protein.) Give the answer to 2 significant figures. A) 70. kcal B) 360 kcal C) 17 kcl D) 630 kcal E) 280 kcal

39) A homogeneous mixture that does not settle out upon standing is A) an element B) a colloid C) a suspension D) solid E) hydrated

4) According to the kinetic theory of gases, particles of a gas A) are very large particles B) are very far apart C) lose their valence electrons D) move slowly E) decrease kinetic energy as temperature increases

40) A slice of pizza contains 28 g of carbohydrate, 13 g of protein and fat. If the pizza contains 280 kcal, how many grams of fat are present?(The caloric values are: 4 kcal/g for carbohydrate, 9 kcal/g for fat, and 4 kcal/g for protein. Give the answer to 2 significant figures.) A) 28 g B) 13 g C) 10. g D) 55 g E) 250 g

40) Consider an isotope of sodium with a mass number of 25. The number of neutrons in this isotope of sodium is A) 11 B) 14 C) 16 D) 25 E) 32

41) The dietary calorie(Cal) is equal to A) 1000 kcal B) 1000 cal C) 100 cal D) 10 cal E) 1 cal

41) What is the mass of 2.00 L of an intravenous glucose solution with a density of 1.15 g/mL? A) 0.0230 kg B) 2.30 kg C) 1.15 kg D) 0.0150 kg E) 0,575 kg

42) The specific heat of a substance is the amount of heat needed to A) change 1 g of the substance from the solid to the liquid state B) raise the temperature of 1 g of the substance by 1 °C C) change 1 g of the substance from the liquid to the solid state D) convert 1 g of a liquid to gas E) convert 1 g of a solid to a gas

47) The specific heat of copper is 0.0920 cal/g °C, and the specific heat of silver is 0.0562 cal/g C. If 100 cal of heat is added to one g of each metal at 25 °C, what is the expected result? A) The copper will reach a higher temperature. B) The silver will reach a higher temperature. C) The two samples will reach the same temperature. D) The copper will reach a temperature lower than 25 °C. E) The silver will soften.

49) What is the element with the electron arrangement 2,8,7? A) Be B) CI C) F D) S E) Ar

5) A mixture is prepared by dissolving 2 g of KCI in 100 g of H20. In this mixture, H2O is the A) solute B) solvent C) solution D) solid E) ionic compound

50) The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called A) osmotic pressure B) dialysis C) solvation D) dilution E) hydration

50) The shape of the methane molecule (CH4) is A) linear B) tetrahedral C) trigonal pyramidal D) bent E) trigonal planar

52) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C? A) 3.6 cal B) 3.6 x 103 cal C) 1.8 cal D) 80, cal E) 0.56 cal

52) The carbon tetrachloride molecule, CCl4, is A) a polar molecule with polar bonds B) a nonpolar molecule with polar bonds C) a nonpolar molecule with nonpolar bonds D) a polar molecule with nonpolar bonds E) a polar molecule with ionic bonds

53) The number of electrons in the outer energy level of a neutral atom of boron (atomic number 5) is A) 2 B) 3 C) 5 D) 8 E) 10

54) The main type of attractive forces between molecules of ammonia (NH3) are A) ionic bónds B) hydrogen bonds. C) polar covalent D) dipole-dipole attractions E) dispersion forces

56) The heat of fusion for water is 80. cal/g. How many calories of heat are released when 20.0 g of water at 0"C is frozen to ice? A) 620 cal B) 1600 cal C) 2000 cal D) 2200 cal E) 0 cal

58) In an electron-dot symbol of an element, the dots are used to represent A) all of the electrons in the atom B) the valence electrons C) the electron arrangement D) only the electrons that will participate in bond formation E) the electrons that the element will gain when it forms a compound

58) The heat of vaporization for water is 540 cal/g. How many kilocalories are needed to change 22 g of liquid water to steam at 100 C? A) 540 kcal B) 12 kcal C) 12000 kcal D) 25 kcal E) 1.8 kcal

63) The atomic size of atoms A) increases going across a period B) decreases going across a period C) decreases going down within a group D) does not change going across a period E) none of the above

65) The ionization energy of atoms A) decreases going across a period B) decreases going down within a group C) increases going down within a group D) does not change going down within a group E) none of the above

66) Ionization energy is A) the energy an ion acquires from an electron B) the energy needed to remove the least tightly bound electron C) highest for metals in Group 1A (1) D) higher for potassium than for lithium E) none of the above

7) The number of electrons in an ion with 16 protons and an ionic charge of 2- is A) 16 B) 18 C) 20 D) 22 E) 24

Classify the following elements. A) alkaline earth metal B) halogen C) noble gas D) transition element E) alkali metal 13) bromine

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 20) 0.9% glucose

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 19) 0.5% NaCl

Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 8) F, S, P

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 16) 1 m=. mm

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 20) 1 kg=. g

Match the type of mixture with the appropriate characteristics. A) solution B) colloid C) suspension 15) a homogeneous mixture in which suspended particles cannot pass through a semipermeable membrane

19) Complete the following statement: In Charles's law, the volume of a gas ——-when the ——-decreases. A) increases, temperature B) increases, quantity of gas C) increases, pressure D) decreases, temperature E) decreases, pressure

19) The mass percent concentration refers to A) grams of solute in 1 kg of solvent B) grams of solute in I kg of solution C) grams of solute in 100 g of solvent D) grams of solute in 100 g of solution E) grams of solvent in 100 g of solution

20) The elements lithium, sodium, and potassium A) are isotopes of each other B) are in the same period of elements C) have the same number of neutrons D) are in the same group E) have the same mass number

25) A sample of argon at 300. °C and 50,0 aun, pressure is cooled in the same container to a temperature of 0.C. What is the new pressure? A) 105 ata B) 45.5 atm C) 54.9 atm D) 23.8 atm E) 42.7 atm

25) Which of the following polyatomic ions has a 3- ionic charge? A) hydroxide B) nitrate C) sulfate D) phosphate E) hydrogen carbonate

26) A conversion factor set up correctly to convert 15 inches to centimeters in A) 100 cm/l m B) 1 inch/2.54 cm C)I cm/10 mm D) 2.54 cm/l inch E) 10 cm/1 inch

27) 9.31 g is the same mass as A) 931 us B) 931 kg C) 93.1 eg D) 9310 mg E) 0.0931 dg

29) What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution? A) 0.500 M B) 1.00 M C)1.50 M D) 2.00 M E) 4.00 M

30) How many moles of CaCl2 are in 250 mL of a 3.0 M of Caa2 solution? A) 750 moles B) 1.3 moles C) 83 moles D) 0.75 mole E) 3.0 moles

30) What is the formula for aluminum nitrate? A) Al2NO2 B) AINO3 C) Al(NO2)3 D) Al(NO3)3 E) Al2(NO2)2

32) In a molecule with covalent bonding, A) oppositely charged ions are held together by strong electrical attractions B) atoms of metals form bonds to atoms of nonmetals C) atoms of different metals form bonds D) atoms are held together by sharing electrons E) atoms of noble gases are held together by attractions between oppositely charged ions

33) A gas sample containing 12 g of CH has a volume of 14 L. What will the volume be if 12 g of He is added? (Temperature and pressure do not change.) A) 22.4. L B) 53 L C) 56 L D) 70 L E) 3.5L

33) Climate change is believed to result from all of the following except A) burning of fossil fuels B) increasing levels of carbon dioxide in the atmosphere C) deforestation D) movement of the earth closer to the sun E) carbon dioxide trapping the heat produced by the sun

33) The number of neutrons in an atom is equal to A) the atomic number B) the mass number C) the mass number + the atomic number D) the mass number - the atomic number E) the number of protons

34) How many moles of neon occupy a volume of 14.3 L at STP? A) 36.7 moles B) 32.0 moles C) 6.45 moles D) 0.638 moles E) 1.57 moles

35) 3.25 kcal is the same amount of energy as A) 3.25 J B) 0.777 J C) 777 J D) 13600 J E) 13.6J

42) The pressure exerted by a gas on its container is directly proportional to A) the volume of the container B) the mass of the individual gas molecules C) the Celsius temperature of the gas D) the number of molecules of gas in the sample E) the Fahrenheit temperature of the gas

45) How many calories are required to raise the temperature of a 150. g sample of gold from 25 °C to 175 °C? The specific heat of gold is 0.0308 cal/g °C. A) 4.62 cal B) 116 cal C) 22500 cal D) 693 cal E) 130. cal

49) Raising the temperature of 10.0 g of water from 10.0 °C to 20.0 °C requires 100.0 cal of of 10.0 g of aluminum from 10.0 °C to 20.0 °C requires energy, while raising the temperature 22.0 cal. More calories are required to heat the water because A) water is a liquid and aluminum is a solid at 10.0 °C B) ten grams of water occupies a larger volume than 10.0 g of aluminum C) water has a greater potential energy than aluminum D) water has a larger specific heat than aluminum E) 10.0 °C is closer to the melting point of water than to the melting point of aluminum

49) The shape of the water molecule (H20) is A) linear B) tetrahedral C) trigonal pyramidal D) bent E) trigonal planar

5) A value of 36 mL is a measure of A) density B) mass C) temperature D) volume E) length

51) The physical state(s) present when a substance is melting is (are) A) solid B) liquid C) gas D) solid + liquid E) liquid + gas

51) What is the electron arrangement for potassium (atomic number 19)? A) 2,8,9 B) 2,8,7,2 C) 2,10,7 D) 2,8,8,1 E) 2,8,6,3

54) What is the correct electron arrangement for the lithium atom? A) 3 B) 3,1 C) 1,2 D) 2,1 E) 2,5

61) The number of dots in the electron dot symbol of carbon is A) one B) two C) three D) four E) five

7) When KCI dissolves in water A) the a- ions are attracted to dissolved K ions B) the a- ions are attracted to the partial negative charge on the oxygen atom of the water molecule C) the K+ ions are attracted to a- ions on the KCI crystal D) the K+ ions are attracted to the partial negative charge on the oxygen atom of the water molecule E) the K* ions are attracted to the partial positive charge on the hydrogen atoms of the water molecule

7) Which measurement describes the pressure of a gas? A) 315 K B) 1.2 g/L. C) 2.5 L D) 725 mmHg E) 0.45 moles

8) Which of the following is not a characteristic of the solid state? A) has a definite shape B) has a definite volume C) particles are close together D) particles are moving very fast E) particles are in fixed positions

9) A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg? A) 1.50 mmHg B) 507 mmHg C) 760 mmHg D) 1140 mmHg E) 3800 mmHg

Classify the following elements. A) alkaline earth metal B) halogen C) noble gas D) transition element E) alkali metal 14) copper

Give the correct mumber of electrons. A) eight B) one Ctwo D) five E) seven 23) in the outer energy level of nitrogen

Give the correct valence for ions of the following elements. A) 3+ B) 2- C) 1- D) 2+ E) 1+ F) 0 1) Ca

Identify the term defined in each description. A) hydration B) unsaturated C) saturated D) hypertonic E) hypotonic F) hydrogen bonding 5) a solution that has a higher osmotic pressure than the red blood cells of the body

Match the statela) of matter with each of the following descriptions of a substance A) liquid B) solid + liquid C) gas D) liquid + gas E) solid 4) This substance is boiling.

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) lengih E) density 18) 1 dl.=. mL

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 2) mm

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 4) kilometer

12) An ionic compound A) has a net positive charge B) has a net negative charge C) contains only cations D) contains only anions E) has a net charge of zero

13) The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming constant temperature? A) 4100 L B) 5.0L c)0.0060 L. D) 5.4 L E) 4.6L

15) Which of the following is a property of a solid? A) It takes the shape of the container. B) It fills the volume of the container. C) The particles move at a rapid rate. D) The interactions between its particles are very weak. E) The particles have fixed positions and are very close together.

16) At constant temperature, a sample of helium at 760. tasg in a closed container was compressed from 5.00 L to 3.00 L. What was the new pressure exerted by the helium a on its container? A) 800. TorrB) 2280 torr C) 15.0 tOrr D) 3800 torr E) 1270 torr

16) In a gas, the distance between the particles is A) very close relative to the size of the molecules B) close relative to the size of the molecules C) fixed relative to the size of the molecules D) small relative to the size of the molecules E) very large relative to the size of the molecules

17) Which of the following elements is a metalloid? A) nitrogen B) lithium C) iron D) gold E) silicon

20) Which of the following is the largest unit? A) millimeter B) micrometer C) meter D) decimeter E) kilometer

21) Rubbing alcohol is 70.% (m/v) isopropyl alcohol by volume. How many mL of isopropyl álcohol are in a 1 pint (473 mL) container? A) 70. mL B) 0.15 ml C) 680 ml. D) 470 mL. E) 330 ml.

21) What is the correct formula for iron(III) sulfide? A) Fe2s2 B) FezS C) EeS D) Feso E) Fe2S3

22) The name of Al2(SO4n is A) aluminum(II) sulfate B) dialuminum trisulfate C) dialuminum sulfate D) dialuminum trisulfide E) aluminum sulfate

24) What volume (mL) of a 15% (m/v) NaOH solution contains 120g 8. NaOH? A) 18 mL B) 0.13 mL C) 13 ml. D) 120 ml. E) 8.0 x 102 ml.

25) How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH? A) 25 mL B) 75 ml. C) 33 ml. D) 19 mL. E) 3.0 x 102 mL.

27) Identify the metalloid in the following list. A) sulfur B) fluorine C) silver D) copper E) germanium

3) What is the symbol for the ion with 19 protons and 18 electrons? A) F+ B) F- C) Art D) K- E) K+

30) According to Avogadro's law, A) the volume of a gas is inversely related to the number of moles at constant temperature and pressure B) the volume of a gas is inversely related to the number of moles at standard temperature and pressure C) the volume of a gas depends only on the temperature and pressure D) the volume of a gas depends only on the number of moles in the sample E) the volume of a gas is directly related to the number of moles at constant temperature and pressure

32) What mass of KCl is in 350 mL of 0.24 M KCI? A) 0.84 g B) 1.1.g C) 84 g D) 18 g E) 6.3 g

33) Which of the following elements does not exist as a diatomic molecule? A) hydrogen B) nitrogen C) chlorine D) охуgеn E) carbon

34) In a covalently bonded molecule, the number of electrons that an atom shares with others is usually equal to the number of electrons A) in the atom B) in its nucleus C) in all the atoms D) in its ion E) needed to give it a noble gas arrangement

35) The correct name of the compound Na3 is A) nitrogen chloride B) trinitrogen chloride C) nitrogen(III) chloride D) nickel chloride E) nitrogen trichloride

35) What volume of 2.5% (m/v) KOH can be prepared from 125 ml of a 5.0% (m/v) KOH solution? A) 0.0040 ml. B) 63 ml. C) 0.10 mL D) 125 ml. E) 250 mL

36) A potato contains 20 g of carbohydrate. If carbohydrate has a caloric value of 4 kcal/g, how many kcal are obtained from the carbohydrate in the potato? A) 5 kcal B) 20 kcal C) 40 kcal D) 60 kcal E) 80 kcal

37) The correct name for the compound N2O3 is A) nitrogen oxide B) nitrogen trioxide C) dinitride trioxide D) dinitrogen oxide E) dinitrogen trioxide

48) Which of the following quantities is not required to calculate the amount of heat energy required to heat water from 25 °C to 55 "C? A) the mass of the water sample B) the initial temperature C) the final temperature D) the specific heat of water E) the heat of vaporization for water

49) A nugget of gold with a mass of 521 g is added to 50.0 mL of water. The water level rises to a volume of 77.0 ml. What is the density of the gold? A) 10.4 g/ml. B) 6.77 g/mL. C) 1.00 g/ml. D) 0.0518 g/ml. E) 19.3 g/ml

54) When a solid is converted directly to a gas, the change of state is called A) freezing B) melting C) boiling D) condensation E) sublimation

55) The main type of attractive forces between molecules of carbon tetrabromide (CBr4) are A) ionic bonds B) hydrogen bonds C) polar covalent D) dipole-dipole attractions E) dispersion forces

56) The main type of attractive forces between molecules of hydrogen (H2) are A) ionic bonds B) hydrogen bonds C) polar covalent D) dipole-dipole attractions E) dispersion forces

60) Which of the following does not involve a change of state? A) melting ice B) freezing water C) vaporization of alcohol D) sublimation of dry ice E) pouring water into a vacuum-insulated bottle

Give the correct valence for ions of the following elements. A) 3+ B) 2- C) 1- D) 2+ E) 1- F) 0 5) K

Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. 7) B

Match the statels) of matter with each of the following descriptions of a substance. A) liquid B) solid + liquid C) gas D) liquid + gas E) solid 3) This material has a definite volume, and a definite shape.

Select the correct prefix to complete the equality. A) 10 B) 1000 C)1 D) 100 E) 0.001. 15) I mL=. L.

Identify the term defined in each description. A) hydration B) unsaturated C) saturated D) hypertonic E) hypotonic F) hydrogen bonding 1) the major attractive forces between water molecules

11) 1 mL is equivalent to 1000 L.

FALSE

12) The density of water is 1 kg/ml.

FALSE

17) An argon atom 18 electrons in the third energy level,

False

18) Ionization energy increases going down a group.

False

18) Molecular compounds are formed from ions.

False

5) Radon is a metal.

False

5) The pressure increases as the volume increases, if temperature does not change.

False

8) The name of the compound AICI3 is aluminum trichloride

False

: 9) To calculate the Kelvin temperature, subtract 273 from the Celsius temperature.

False

Condensation occurs when a liquid is converted to a solid.

False

14) The amount of heat necessary for one point is the gram of a substance to change from the solid state to the liquid state at its melting point is the —

Heat of fusion

18) If a red blood cell is placed in 1% glucose solution, the red blood cell will

Hemolyze

7) When MgQ. is added to water, the salt will be

Insoluble

Identify each of the following compounds as covalent or ionic 2) potassium oxide

Ionic

Identify each of the following compounds as covalent or ionic 5) sodium fluoride

Ionic

13) The heat of fusion is the amount of heat necessary to change one gram of a substance from the solid to the —state at its melting point.

Liquid

Bramine (Brz) has a freezing point of -7 °C, and a boiling point of 60 °C. Indicate the state present or the change of state occurring at each temperature. 16) 30 °C

Liquid

Write the symbol from the element name. 5) The symbol for sulfur is

1) The air we breathe is about 21% oxygen.

TRUE

11) In deoxygenated blood, the partial pressure of carbon dioxide is greater than the partial pressure of oxygen left.

TRUE

13) Specific gravity has no units.

TRUE

2) The liter is a unit of volume in the metric system.

TRUE

3) The kinetic energy of a gas sample is directly proportional to the Kelvin temperature of the gas.

TRUE

6) Gas law calculations require the use of the Kelvin temperature scale.

TRUE

6) When the measured number 675 is added to the measured number 87.10, the answer should be rounded to the ones place.

TRUE

8) The volume of 1 mole of any gas at STP is 22.4 L.

TRUE

8) There are 1000 ug in a mg.

TRUE

9) STP stands for 0 °C and 760 mmHg.

TRUE

17) When a liquid is boiling, its temperature does not change.

True

18) As a solid melts, its temperature does not change.

True

19) Metallic character increases going down a group.

True

19) The formula of the compound boron trifluoride is BF3.

True

2) Black coffee is a homogeneous mixture.

True

20) Atomic size decreases going from left to right within a period.

True

20) The temperature at which water melts and freezes is the same.

True

22) Chlorine is more electronegative than bromine.

True

22) Potassium has one valence electron.

True

24) The bond between H and O is polar covalent.

True

26) The molecule CO2 is linear.

True

29) Ammonia, (NH3), is a polar molecule.

True

3) A positive ion has more protons that electrons.

True

30) A nonpolar molecule can have polar bonds.

True

32) The strongest attractive forces between molecules of Cl2 are dispersion forces.

True

33) The strongest attractive forces between molecules of NH3 are hydrogen bonds.

True

35) The strongest attractive forces between molecules of HBt are dipole-dipole attractions.

True

4) At 0 K, all molecular motion stops.

True

4) Chromium is a metal.

True

5) Iron rusting is a chemical change.

True

5) When calcium and oxygen combine, the formula of the product is CaQ.

True

7) Sulfur is a nonmetal.

True

8) An object with a temperature of 20. °C is hotter than another object with a temperature of 20. °F.

True

9) The proton has a positive charge.

True

6) Mercury is a metal.

Truw

17) If a red blood cell is placed in 5% NaCl solution, the red blood cell will

crenate

) A substance that carries an electric current when dissolved in water is called a(n)

electrolyte

Bramine (Brz) has a freezing point of -7 °C, and a boiling point of 60 °C. Indicate the state present or the change of state occurring at each temperature. 18) -7 °C

melting or freezing

6) When barium and chlorine combine, the formula of the product is BaCl3.

False

7) When A13+ and Br combine, the formula of the product is Al3Br.

False

8) Iodine is a metal.

False

9) A cubic centimeter is a unit of length.

False

Carbohydrates and proteins have the same caloric value per gram.

True

Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 7) Li, C, F

42) Which of the following compounds contains a polar covalent bond? A) Nal B) HCL C) Br2 D) MgQ E) o

48) Which solution is isotonic to a red blood cell? A) water B) 0.5% NACI C) 2% glucose D) 0.9% NaCI E) 10% glucose

20) The name of the compound CO2 is dicarbon oxide.

False

21) Br2 contains a polar covalent bond.

False

21) Sulfur has 16 valence electrons.

False

Round off each of the following to three significant figures. 7) 0.003 4088

0.00341

5) How many equivalents are in 0.036 mole of Ca2+?

0.072 equivalents

34) The strongest attractive forces between molecules of HCl are hydrogen bonds.

False

4) The pressure unit 1 mmHg is the same pressure unit as the pressure unit—

1 torr

Write the electron arrangement for the atom shown. 7) Sodium

2,8,1

Write the electron arrangement for the atom shown. 11) Magnesium

2,8,2

Write the electron arrangement for the atom shown. 12) Phosphorus

2,8,5

Write the electron arrangement for the atom shown. 10) Sulfur

2,8,6

Write the electron arrangement for the atom shown. 8) Chlorine

2,8,7

Write the electron arrangement for the atom shown. 9) Argon

2,8,8

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells . A) hypertonic B) hypotonic C) isotonic 21) 7% glucose

15) Which has a higher osmotic pressure 1.0 M sucrose or water?

1.0 M sucrose

13) When 50. mL of 1aa (m/v) NaCl is diluted to 500. mL, the NaCl concentration is —-%.

1.0% (m/v)

11) A gas has a volume of 45.0 L and a pressure of 540. mmHg when the temperature is 27 °C. What is the volume when the pressure changes to 800, mmHg with a temperature of -65 °C, if there is no change in the amount of gas?

21.1 L

14) The correct formula for the compound formed from Mg and S is A) MgS B) Mg52 C) Mg28 D) Mg252 E) Mg253

4) For halogens, the group number is the same as the ionic charge.

False

19) What is the correct formula for the iron(II) ion? A) Fet B) Fe2+ C) Fe D) F2- E) Fe3-

26) What is the molarity of a solution that cotains 17 g of NH3 in 0.50 L of solution? A) 34 M B) 2.0 M C) 0.50 M D) 0.029 M E) 1.0 M

44) lonic bonding is expected in which of these compounds? A) a2 B) KF c) OF2 D) HF E) H2

45) A liquid has a volume of 34.6 mL and a mass of 46.0 g. What is the density of the liquid? A) 1.00 g/mL B) 1.33 g/ml. C) 0.752 g/mL D) 1330 g/mL E) 0.663 g/ml

46) The bond in Cy is a(n) A) ionic bond B) nonpolar covalent bond C) metallic bond D) polar ionic bond E) no bond

47) Diamond has a density of 3.52 g/ml. What is the volume in cubic centimeters of a diamond with a mass of 15.1 g? A) 4.3 cm B) 4.29 cm C) 0.233 cm D) 53 cm E) 53.2 cm

1) Acetic acid can be classified as a A) gas B) solid C) weak electrolyte D) strong electrolyte E) ionic compound

1) The primary substances of which all other things are composed are A) molecules B) compounds C) elements D) electrons E) protons

12) Which of the following is a characteristic of the modern periodic table? A) A group is a horizontal row on the periodic table. B) A period is a column on the periodic table. C) The elements in each group have similar chemical properties. D) The B groups contain the representative elements. E) The A groups contain the transition elements.

36) What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A) 0.075 L B) 0.25 L C) 0.75 L D) 0.083 L E) 750 L

4) Gold in a ring is a(n) A) compound B) heterogeneous mixture C) element D) homogeneous mixture E) none of the above

4) Which of the following molecules can form hydrogen bonds? A) CH4 B) NaH C) NH3 D) BH3 E) HI

41) Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of 118/50 Sn? A) 118 protons, 50 neutrons, 118 electrons B) 118 protons, 118 neutrons, 50 electrons C) 50 protons, 68 neutrons, 50 electrons D) 68 protons, 68 neutrons, 50 electrons E) 50 protons, 50 neutrons, 50 electrons

3) Iron rusting is an example ofa — change

Chemic

16) —-can pass through filters but cannot pass through semipermeable membranes.

Colloids

11) Which of the following is a chemical change? A) cutting a rope B) bending a steel rod C) making a snowman D) burning sugar E) melting gold

13) Which of the following properties is not a characteristic of the Group 1A (1) elements (alkali metals)? A) They are shiny. B) They are good conductors of heat. C) They react vigorously with water. D) Most of them are liquids at room temperature. E) They are good conductors of electricity.

15) The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H20, A) all of the KI will dissolve B) the solution will freeze C) the solution will start boiling D) a saturated solution will form E) the solution will be unsaturated

15) Which of the following elements is a metal? A) nitrogen B) fluorine C) argon D) strontium E) phosphorus

26) Absolute zero is A) the freezing point of water using the Celsius scale B) the boiling point of liquid nitrogen C) the temperature on the Kelvin scale corresponding to 32 °F D) the coldest temperature possible E) the freezing point of liquid nitrogen

1) In ionic compounds, ——lose their valence electrons to form positively charged —— A) metals, anions B) nonmetals, cations C) metals, polyatomic ions D) nonmetals, anions E) metals, cations

1) The amount of space occupied by a substance is its A) mass B) density C) weight D) length E) volume

5) An anion always — A) has a positive charge B) contains a group of two or more atoms with a positive charge C) contains a metal and a nonmetal D) forms covalent bonds E) has a negative charge

When a liquid boils, the process by which the molecules leave its surface is called —

Evaporation

17) If there are 14 books on the shelf, 14 is a(n) number.

Exact

car driving on the freeway has—- energy.

Kinetic

Write the symbol from the element name. 2) The symbol for lead is

2) Liquid water changing to ice is an example of a

Physical

1) Polar solutes are soluble in —— solvents.

Polar

8) A bungee jumper just before she leaps, has —energy.

Potential

4) The state of matter has a constant shape and volume.

Solid

Bramine (Brz) has a freezing point of -7 °C, and a boiling point of 60 °C. Indicate the state present or the change of state occurring at each temperature. 19) -15 °C

Solid

6) When KCI is added to water, the salt will be

Soluble

4) A substance that completely ionizes in water is a —— electrolyte.

Strong

1) The symbol for gold is Au.

True

3) A substance that produces only a small number of ions in solution is known as a ——electrolyte.

Weak

8) When NH4C1 is added to water, the salt will be

soluble

The change of state from solid to gas is termed

sublimation

11) Which of the following correctly describes the process of inspiration (air entering the lungs)? A) The lungs expand, causing their internal pressure to decrease. B) The lungs expand, causing their internal pressure to increase. C) The lungs contract, causing their internal pressure to decrease, D) The lungs contract, causing their internal pressure to increase. E) There is no change in the internal pressure in the lungs.

12) How many equivalents are in 0.40 mole of K? A) 0.40 Eg B) 0.80 Eq C) 0.20 Eg D) 2.0 Ea E) 1.0 Eg

14) The Group 8A (18) elements A) are unreactive and are rarely found in combination with other elements B) are good conductors of electricity C) melt at high temperatures D) are liquids at room temperature E) react vigorously with water

16) What is the correct formula for the oxide ion? A) 02- B) O C) O D) 02. E) o+

2) Au is the symbol for A) gold B) silver C) argon D) aluminum E) sodium

2) Which of the following is the basic unit of volume in the metric system? A) liter B) kilogram C) meter D) centimeter E) gram

21) If the temperature is -55 °F, what is the corresponding temperature on the Kelvin scale? A) 225 K B) 218 K C) 55 K D) 273 K E) 328 K

23) The temperature of liquid nitrogen is -196 °C. What is the corresponding reading on the Kelvin scale? A) 77 K B) -127 K C) -91 K D) 48 K E) 146 K

25) A temperature of 41 °F is the same as A) 5 °C B) 310 °C C) 9 °C D) 16 °C E) 42 °C

25) Identify the noble gas in the following list. A) helium B) nitrogen C) oxygen D) gold E) chlorine

27) A sample of nitrogen gas had a volume of 500. ml., a pressure in its closed container of 740 too, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 tog? A) 530 ml. B) 450 ml C) 970 ml. D) 240 mL E) 400 ml.

27) The molarity (M) of a solution refers to A) moles of solute/L of solution B) moles of solute/ L of solvent C) moles of solute/100 mL of solution D) grams of solute/100 mL of solution E) grams of solute/L of solution

28) At 570. mmHg and 25 "C, a gas sample has a volume of 2270 ml What is the final pressure (in mmiig) at a volume of 1250 ml. and a temperature of 175 C? A) 1560 mmHg B) 210 mmHg C) 7000 mmlg D) 690 mmHg E) 470 mmHg

28) What is the formula of a compound that contains Nat and PO3- ions? A) Na3PO4 B) NaPO4 C) NazPO3 D) NagPO3 E) NazP

28) What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution? A) 2.5 M B) 1.0 M C) 5.0 M D) 10. M E) 2.0 M

29) 1.00 pint of milk has a volume of how many milliliters? A) 473 ml. B) 530. ml. C) 1000 ml. D) 1890 ml. E) 106 ml.

3) In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules A) move rapidly in random directions B) are attracted to each other by strong forces C) are close together in their container D) move with a kinetic energy equal to their centigrade temperature E) occasionally come to rest

30) Which of the following descriptions of a subatomic particle is correct? A) A proton has a positive charge and a mass of approximately 1 amu. B) An electron has a negative charge and a mass of approximately 1 amu. C) A neutron has no charge and its mass is negligible. D) A proton has a positive charge and a negligible mass. E) A neutron has a positive charge and a mass of approximately 1 amu.

33) 5.21 cm is the same length as A) 0.0521 m B) 52.1 dm C) 5.21 mm D) 0.00521 km E) 5210 m

33) During the process of diluting a solution to a lower concentration, A) the amount of solute does not change B) the amount of solvent does not change C) there is more solute in the concentrated solution D) the volume of the solution does not change E) water is removed from the concentrated solution

34) 650. J is the same amount of energy as A) 155 cal B) 2720 ca. C) 650. cal D) 1550 cal E) 2.72 cal

36) Consider a neutral atom with 30 protons and 34 neutrons. The atomic number of the element is A) 30 B) 32 C) 34 D) 64 E) 94

36) How many kilograms are in 30.4 1b? A) 13.8 kg B) 14 kg C) 67 kg D) 66.88 kg E) 66.9 kg

38) Consider a neutral atom with 30 protons and 34 neutrons. The number of elcctrons in this atom is A) 30 B) 32 C) 34 D) 64 E) 94

38) What is the new mass/volume percent (m/v) of a KOH solution that is prepared by diluting 110 mL of a 6.0% (m/v) KOH solution to 330 mL? A) 2.0% (m/v) B) 1.0% (m/v) C) 6.0% (m/v) D) 12% (m/v) E) 18% (m/v)

39) A tank contains helium gas at 490 mmHg, nitrogen gas at 0.7S atm, and neon at 520 torr What is the total pressure in atu? A) 2.1 atm B)0.55 atm C) 1.0x10^3atm D) 1.5 atm E) 1600 atm

39) How many protons are in an isotope of sodium with a mass number of 25? A) 11 B) 14 C) 15 D) 25 E) 32

39) The ability of an atom to attract the shared electrons in a covalent bond is its A) electronegativity B) bonding ability C) polarity D) ionic character E) nonpolatity

39)'A serving of fish contains 50 g protein and 4 g of fat. If protein has a caloric value of 4 kcal/g and fat has 9 kcal/g, how many kcal are in the serving? Give the answer to 2 significant figures. A) 240 kcal B) 54 kcal C) 470 kcal D) 220 kcal E) 490 kcal

40) Which of the following correctly describes the partial pressures of gases in the body? A) high o2, low co2, oxygenated blood B) high O2, low co2, deoxygenated blood C) high o2, high Co2, oxygenated blood D) high o2, high co2, tissue E) low O2, low co2, deoxygenated blood

44) How many calories are required to raise the temperature of a 35.0 g sample of iron from 25 °C to 35 °C? Iron has a specific heat of 0.108 cal/g °C. A) 38 cal B) 1.1 cal C) 3.8 cal D) 93 cal E) 130 cal

45) A 10% starch solution is separated from a 2% starch solution by a semipermeable membrane. Starch is a colloid. Which of the following is correct? A) The 10% solution has the higher osmotic pressure. B) The 2% solution has the higher osmotic pressure. C) Neither solution has osmotic pressure. D) The solutions have the same osmotic, pressure. E) The solutions have opposite osmotic pressures.

45) A polar covalent bond is found in which of these compounds? A) H20 B) F2 C) NaCI D) H2 E) Na

46) Which of the following is not true for the atoms 13N, 14N, and 15N? A) They all have the same mass number. B) They are isotopes. C) They all have the same atomic number. D) They all have 7 protons. E) They all have 7 electrons.

47) The VSEPR theory allows us to determine the A) shape of molecule B) charge on an ion C) color of a compound D) bond type for a molecule E) formula for a compound

49) A red blood cell will undergo hemolysis in A) water B) 0.9% NaCi C) 5% glucose D) 5% NaCi E) 10% glucose

50) What is the electron arrangement for aluminum? A) 2,8,3 B) 2,8,5 C) 2,8,7 D) 2,8,8 E) 2,8,10

51) The carbon tetrachloride molecule, CCl4, has the shape of a A) tetrahedron B) square C) cube D) circle E) sphere

53) The ammonia molecule (NH3) is A) a polar molecule with polar bonds B) a nonpolar molecule with polar bonds C) a nonpolar molecule with nonpolar bonds D) a polar molecule with nonpolar bonds E) a polar molecule with ionic bonds

53) The formation of a gas resulting from the escape of high-energy particles from the surface of a liquid is known as A) evaporation B) deposition C) boiling D) melting E) sublimation

57) Valence electrons are electrons located A) in the outermost energy level of an atom B) in the nucleus of an atom C) in the innermost energy level of an atom D) throughout the atom E) in the first three shells of an atom

6) The force of gas particles against the walls of a container is called A) pressure B) volume C) temperature D) quantity of gas E) density

63) Which of the following does not represent a step on the heating curve of water? A) The temperature of steam cannot exceed 100 °C. B) The temperature of ice remains at 0 "C as it melts. C) The temperature of liquid water increases tinearly as it is heated. D) The temperature of liquid water remains at 100 °C as it boils. E) Both liquid water and ice are present at 0 "C.

68) The metallic character of elements A) decreases going across a period B) decreases going down within a group C) increases going across a period D) does not change going down within a group E) none of the above

9) Which of the following is an example of a physical change? A) grinding coffee beans B) baking a cake C) converting water to hydrogen and oxygen D) digesting a cheeseburger E) buming coal

Classify the following elements as metals, metalloids, or nonmetals. A) metal B) nonmetal C) metalloid 19) cobalt

Classify the following elements as metals, metalloids, or nonmetals. A) metal B) nonmetal C) metalloid 21) nickel

Classify the following elements as metals, metalloids, or nonmetals. A) metal B) nonmetal C) metalloid 22) potassium

Classify the following elements. A) alkaline earth metal B) halogen C) noble gas D) transition element E) alkali metal 15) magnesium

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 22) 5% NaCI

For the following question(s), consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. 41) Which starch solution will decrease in volume as osmosis occurs? A) 4% B) 10% C) Neither exerts osmotic pressure. D) They exert equal osmotic pressures. E) They exert opposite osmotic pressures.

Give the correct valence for ions of the following elements. A) 3+ B) 2- C) 1- D) 2+ E) 1+ F) 0 4) Al

Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. 10)E

Identify the term defined in each description . A) hydration B) unsaturated C) saturated D) hypertonic E) hypotonic F) hydrogen bonding 2) the association of several water molecules with ions produced in a solution

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 3) The volume and the Kelvin temperature are reduced by one-half (n constant)

Indicate the type of bonding you would expect between the following elements. A) ionic B) polar covalent C) none D) nonpolar covalent 20) Na and F

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 11) glucose, a nonelectrolyte

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 7) urea, a nonelectrolyte

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 9) CH3CH2OH, a nonelectrolyte

Match the chemical name with the correct formula. A) Mg(HSO4)2 B) MgSO4 C) MgS D) Mg(HSO3)2 E) MgS03 16) magnesium hydrogen sulfate

Match the statels) of matter with each of the following descriptions of a substance. A) liquid B) solid + liquid C) gas D) liquid + gas E) solid 1)Particles are held close together in a random pattern.

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 17) 1 cm = mm

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 3) gram

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 5) milligram

Match the type of mixture with the appropriate characteristics. A) solution B) colloid C) suspension 13) a mixture of sodium chloride in water

Match the type of mixture with the appropriate characteristics. A) solution B) colloid C) suspension 16) a mixture whose particles cannot be separated by filters or semipermeable membrunes

Bramine (Brz) has a freezing point of -7 °C, and a boiling point of 60 °C. Indicate the state present or the change of state occurring at each temperature. 20) 70 °C

gas

12) The number of moles of a compound dissolved in one liter of a solution is called the

molarity

37) What volume of a 2.00 M KCI solution is required to prepare 500. mL of a 0.100 M KCI solution? A) 0.0400 mL. B) 25.0 ml. C) 2.00 ml. D) 1.00 x 104 mL E) 5.00 x 102 mL

38) What is the formula of carbon tetcaiodide? A) CI B) Cl4 C) CI D) C3 E) C24

For the following question(s), consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. 43) Which of the following also occurs in this system? A) Water flows equally in both directions. B) There is a net flow of water from the 4% starch solution into the 10% starch solution . C) There is a net flow of water from the 10% starch solution into the 4% starch solution. D) Water does not cross the membrane at all. E) Starch moves out of the 10% starch solution into the 4% starch solution.

Give the correct number of electrons. A) eight B) one C) two D) five E) seven 27) in the third energy level of sodium

Give the correct valence for ions of the following elements. A) 3+ B) 2- C) I- D) 2+ E) I+ F) 0 3) O

Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. 8) c

Identify the term defined in each description. A) hydration B) unsaturated C) saturated D) hypertonic E) hypotonic F) hydrogen bonding 4) a solution in which more solute can be dissolved

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 1) decrease in volume (n, T constant)

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 2) The temperature is doubled. (Ka constant)

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 6) One mole of gas is added V,T constant)

Indicate the type of bonding you would expect between the following elements. A) ionic B) polar covalent C) none D) nonpolar covalent 24) S and F

Indicate the type of bonding you would expect between the following elements. A) ionic B) polar covalent С) попе D) nonpolar covalent 21)N and F

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 12) H2CO3, a weak electrolyte

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 8) HF, a weak electrolyte

2) The molarity of a solution of 5.0 g of KCl in 100. mL of solution is A) 0.038 M B) 0.067 M C) 0.67 M D) 0.13 M E) 1.3 M

23) A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound B) anion C) polyatomic ion D) cation E) molecule

23) How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution? A) 800. g B) 0.0050 g C) 8.0 8 D) 2.0 g E) 200. g

23) The cubic centimeter (Cm3 or cc) has the same volume as a A) cubic inch B) cubic liter C) milliliter D) centimeter E) cubic decimeter

24) On a hot day, the thermometer read 95 "F. What is the temperature in degrees Celsius? A) 77 °C B) 113 °C C) 35 °C D) 63 °C E) 178 °C

26) A gas at 5.00 ata pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank in the summer? A) 0.625 atm B) 4.44 atm. C) 5.63 atm. D) 40.0 atm E) 69.5 atm

26) Semiconductors are located in the periodic table on (or in) the A) left side of the table B) right side of the table C) line dividing metals from nonmetals in the table D) first period of the table E) last period of the table

28) According to the United States Food and Drug Administration, the recommended daily requirement of protein is 44 g. This is of protein. A) 1248.5 oz B) 320 000 oz C) 1.6 oz D) 0.0605 oz E) 150 000 oz

28) The energy associated with the motion of particles in a substance is calied A) temperature B) electrical energy C) heat D) chemical energy E) potential energy

29) Fe2(SO4)3 is called A) iron sulfate B) iron(II) sulfate C) iron(III) sulfate D) diiton trisulfate E) iron trisulfate

3) Which of the following is a measurement of mass in the metric system? A) milliliter B) centimeter C) kilogram D) Celsius E) meter

30) Which of the following setups would convert centimeters to feet?

31) A(n) —is the smallest neutral unit of two or more atoms held together by a covalent bond. A) ionic compound B) nucleus C) molecule D) formula E) unit

32) A gas sample contains 4.0 g of CH4 and 2.0 g of He. What is the volume of the sample at STP? A) 130 L B) 11L C) 17 L D) 30. L E) 5.6 L

32) How many liters of soft drink are there in 5.25 qr? A) 4950 L B) 55.7L C) 4.95 L D) 5.57 L E) 5.0 L

47) The electron arrangement of any particular atom shows A) the number of isotopes possible B) a description of the shape of each electron energy level C) the number of electrons in each energy level D) a diagram of an atomic nucleus E) the maximum number of electrons cach energy level can hold

48) The shape of the ammonia molecule (NH3) is A) linear B) trigonal planar C) trigonal pyramidal D) tetrahedral E) bent

50) The number of calories needed to raise the temperature of 32 g of water from 12 Cto 54 CIs A) 380 cal B) 1.3 cal C) 1300 cal D) 1700 cal E) 0.76 cal

Classify the following elements as metals, metalloids, or nonmetals A) metal B) nonmetal C) metalloid 18) germanium

Classify the following elements. A) alkaline earth metal B) halogen C) noble gas D) transition element E) alkali metal 12) argon

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 24) 0.9% NaCI

Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) hypotonic C) isotonic 23) 5% glucose

Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 6) Li, Na, K

Do the following represent elements in a group, a period, or neither? A) period B) neither C) group 9) 0, S, Se

Give the correct number of electrons. A) eight B) one C) two D) five E) seven 26) in the first electron energy level of chlorine

Give the correct valence for ions of the following elements. A) 3+ B) 2- C) 1- D) 2+ E) 1+ F) 0 2) CI

Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. 9)D

Identify the term defined in each description. A) hydration B) unsaturated C) saturated D) hypertonic E) hypotonic F) hydrogen bonding 3) a solution that contains the highest amount of solute that dissolves at a given temperature :

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 4) removing some molecules of gas (K.T constant)

Indicate the effect of each change upon the pressure of a gas. A) no change B) increases C) decreases 5) A leak occurs and gas escapes.(V.T constant)

Indicate the type of bonding you would expect between the following elements. A) ionic B) polar covalent C) none D) nonpolar covalent 23) He and F

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both . A) molecules B) both C) ions 6) NaCL a strong electrolyte

Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) molecules B) both C) ions 10) KNO, a soluble salt

Identify each of the following compounds as covalent or ionic 3) carbon dioxide

Covalent

Identify each of the following compounds as covalent or ionic 4) dihydrogen sulfide

Covalent

Identify each of the following compounds as covalent or ionic 6) nitrogen trichloride

Covalent

Write the symbol from the element name. 4) The symbol for copper is

10) Which of the following would not be a physical change? A) freezing water to make ice cubes B) tearing a piece of aluminum foil C) boiling water for soup D) burning gasoline in a lawnmower E) melting gold to make jewelry

11) When a cation is formed from a representative element A) electrons are gained and the ion is larger B) electrons are gained and the ion is smaller C) electrons are lost and the ion is larger D) electrons are lost and the ion is smaller E) the cation acquires a negative charge

16) When 2610+ 11.7+0.22 are added, the answer to the correct number of decimal places is A) 2621.92 B) 2621.9 C) 2621 D) 2620 E) 2600

17) The compound MgC2 is named A) magnesium chlorine B) magnesium dichloride C) magnesium(I) chloride D) magnesium chloride E) dimagnesium chloride

17) What is the answer, with the correct number of decimal places, for this problem? 4.392 g+ 102.40 g+ 2.51 g- A) 109.302 g B) 109 g C) 109.3 g D) 109.30 g E) 110 g

17) Which of the following is a physical property of both liquids and gases? A) has its own shape B) has a definite volume C) has strong interactions between its particles D) has randomly arranged particles E) has large spaces between molecules

18) Which of the following is a characteristic of nonmetals? A) shiny B) malleable C) good conductors of heat D) low melting points E) good conductors of electricity

19) Which of the following elements is a noble gas? A) охудеn B) chlorine C) bromine D) argon E) nitrogen

2) How many electrons will aluminum gain or lose when it forms an ion? A) lose I B) gain 5 C) lose 2 D) lose 3 E) gain 1

20) What is the concentration, in mass percent (m/m), of a solution prepared from 50.0 g NeC and 150.0 g of water? A) 0.250% (m/m) B) 33.3% (m/m) C) 40.0% (m/m) D) 25.0% (m/m) E) 3.00% (m/m)

22) A patient has a temperature of 38.5 °C. What is the temperature in degrees Fahrenheit? A) 70.5 °F B) 311 °F C) 126.9 °F D) 101.3 °F E) 11.7 °F

23) What is the symbol of the element in Group 4A (14) and Period 2? A) Be B) Mg C) Ca D) C E) Si

24) Agas contained in a steel tank has a pressure of 1.5 au at a temperature of 320 K. What wil be the gas pressure when the temperature changes to 450 K7 A) 1.5 atm. B) 0.94 atm C)0.47 atm D) 2.1 atm E) 1.1 atm

24) The element in this list with chemical properties similar to magnesium is A) sodium B) boron C) carbon D) strontium E) chlorine

24) Which of the following polyatomic ions has a positive charge? A) hydroxide B) cyanide C) hydrogen carbonate D) ammonium E) nitrate

25) Which of the following conversion factors is a measured number? A) 10 cm/dm B) 12 in/f C) 16 oz/lb D) 25 miles/gallon E) 12 eggs/dozen

35) What is 6.5 m converted to inches? A) 1700 in B) 1651 in C) 39 in D) 260 in E) 255.9 in

35) What is the mass number of an atom of potassium that has 20 neutrons? A) 15 B) 19 C) 35 D) 39 E) 59

36) According to naming rules, the types of compound that use prefixes in their names are A) ionic compounds B) ionic compounds involving transition metals C) polyatomic ions D) molecular compounds E) compounds that contain polyatomic ions

37) Consider a neutral atom with 30 protons and 34 neutrons. The mass number for this atom is A) 30 B) 32 C) 34 D) 64 E) 94

37) One cup of kidney beans contains 15 g of protein, 1 g of fat, and 42 g of carbohydrate. How many kilocalories, to two significant figures, does this sample contain? (The caloric values are: 4 kcal/g for carbohydrate, 9 kcal/g for fat, and 4 kcal/g for protein.) A) 60. kcal B) 88 kcal C) 230 kcal D) 240 kcal E) 520 kcal

4) To form an ion, a sodium atom — A) gains one electron B) gains two electrons C) loses seven electrons D) loses one electron E) loses two electrons

40) In the process known asOsmosis, ————moves through a semipermeable membrane into an area of ———-concentration. A) solute, lower solute B) solute, higher solute C) solvent, lower solute D) solvent, lower solvent E) solvent, higher solvent

42) Isotopes are atoms of the same element that have A) different atomic numbers B) the same atomic numbers but different numbers of protons C) the same atomic numbers but different numbers of electrons D) the same atomic number but different numbers of neutrons E) the same atomic mass but different numbers of protons

42) Mercury has a specific gravity of 13.6. How many milliliters of mercury have a mass of 0.35 kg? A) 0.0257 ml. B) 0.026 ml. C) 25.7 ml D) 26 mL E) 4760 mL

43) A kilocalorie of heat is required to raise the temperature of A) 1 g of water from 14 °C to 15 °C B) 1 g of water by 10 °C C) 10 g of water by 10 °C D) 100 g of water by 10 °C E) 100 g of water by 100 °C

44) The atomic mass of an element is equal to A) its mass number B) its atomic number C) one-twelfth of the mass of a carbon-12 atom D) the mass of an "average atom" E) the mass of the heaviest isotope

45) A sample of chlorine has two naturally occurring isotopes. The isotope Cl-35 makes up 75.8% of the sample, and the isotope Cl-37 makes up 24.3% of the sample. Which of the following statements is true? A) The atomic mass of chlorine will be less than 35. B) The atomic mass of chlorine will be more than 37. C) You cannot tell what the atomic mass will be. D) The atomic mass will be between 35 and 37, E) The atomic mass will be 24.3.

45) At STP, what is the volume of 1.0 mole of carbon dioxide? A) 1.00 L B) 44.0 L C) 273 L D) 22.4 L. E) 12.2L

46) A solution that has an osmotic pressure less than that of red blood cells is called A) saturated B) hypertonie C) isotonic D) hypotonic E) unsaturated

61) A heating curve illustrates A) what a substance looks like as it is heated B) what happens to the particles of a substance as it is heated C) what happens to the heat applied as the temperature is increased D) the changes in the temperature and physical state of a substance as it is heated E) the chemical changes that occur as the substance is heated

62) On a heating curve a plateau corresponds to A) a change in temperature of a liquid B) a change in temperature of a solid C) a change in temperature of a gas D) a change of state E) the solid being broken into smaller pieces

Indicate the type of bonding you would expect between the following elements. A) ionie B) polar covalent C) none D) nonpolar covalent 22) F and F

Match the chemical name with the correct formula. A) Mg(HSO42 B) MgS04 C) MgS D) Mg(HSO32 E) MgSO) 19) magnesium hydrogen sulfite

Select the correct symbol for the element named. 6) mercury A) Mr B) Na C) Au D) Hg E) Ag

Select the correct symbol for the element named. 9) gold A) Go B) Hg C) Ag D) Au E) AU

10) In response to Boyle's law, the pressure of a gas increases as the volume decreases because A) the gas particles get bigger B) the kinetic energy of the gas particles increases C) the temperature of the gas increases D) the gas particles strike the walls of the container with more force E) the gas particles strike the walls of the container more often

13) The correct formula for a compound formed from the elements Al and O is A) AlQ. B) Al20 C) Al302 D) Alos E) Al203

37) The total pressure in a mixture of gases is equal to the partial pressure(s) of A) the gas with the greatest number of moles B) the gas with the smallest number of moles C) the gas with the highest molecular weight D) the gas that occupies the largest volume E) all the gases added together

38) A cyclopropane-oxygen mixture is used a an anesthetic. Ifthe partial pressure of cyelopropane in the mixture is 330 mmHg and the partial pressure of the onygen is 1.0 atm, what is the total preaaure of the misture in tore?A) 330 torr B) 430 torrC) 760 torrD) 1.4 torr E) 1100 torr

41) Which of the following substances contains a nonpolar covalent bond? A) H20 B) NaCI C) NH3 D) MgF2 E) N2

44) Al STP, how many moles of helium would occupy 1.00 L? A) 2.24 moles B) 224 moles C) 22.4 moles D) 0.446 moles E) 0.0446 moles

47) A red blood cell will undergo crenation in A) water B) 0.5% NaCl C) 3% glucose D) 5% glucose E) 7% NACI

60) The number of dots in the electron dot symbol of nitrogen is A) one B) two C) three D) four E) five

8) The unit of 1 atmosphere used to describe the pressure of a gas is equal to A) 1 mmHg B) 100 mmHg C) 200 mmHg D) 600 mmHg E) 760 mmHg

Classify the following elements. A) alkaline carth metal B) halogen C) noble gas D) transition element E) alkali metal 11) sodium

For the following question(s), consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. 42) The process that occurs in this system is A) filtration B) hydration C) neutralization D) dialysis E) osmosis

Give the correct number of electrons. A) eight B) one C) two D) five E) seven 25) in the highest occupied electron energy level of chloine

Match the chemical name with the correct formula. A) Mg(HSO412 B) MgS04 C) MgS D) Mg(HSO3)2 E) MgS03 18) magnesium sulfite

Identify the physical state )corresponding to labeled regions on the cooling curve of water shown below. A) solid B) liquid C) liquid and solid D) solid and gas E) liquid and gas 6) A

10) During inspiration, we use 100% of the oxygen in the air we breathe.

FALSE

2) The speed of gas molecules is related to the volume of the container.

FALSE

7) A ug is larger than a mg.

FALSE

7) The pressure exerted by a gas on its container is inversely related to its Kelvin temperature.

FALSE

The basic unit of mass in the metric system is the pound.

FALSE

1) Air is a heterogeneous mixture.

False

10) The proton is 2000 times the mass of the neutron.

False

13) One gram of fat has less energy that one gram of protein

False

13) The atomic number of sodium is 23.

False

14) A sodium atom with a mass number of 23 has 23 neutrons.

False

14) The specific heat has units of kcal.

False

15) The heat of fusion is greater than the heat of vaporization,

False

16) The name of the compound CuSO4 is copper(I) sulfate.

False

19) Steam at 100 "C contains the same amount of heat as liquid water at 100 °C.

False

2) A potassium atom gains electrons to form an ion with a charge of 1-.

False

23) Sodium is more electronegative than chlorine.

False

27) The molecule SC12 is linear.

False

28) Methane, (CH4), is a polar molecule.

False

31) The strongest attractive forces between molecules of H20 are dispersion forces.

False

9) The common ions of iron are Fet and Fe2+.

False

I1) The name of the compound Fe2S3 is iron(II) sulfide.

False

26) What is the formula of the nitride ion? A) N3- B) NO2" C) NO3- D) NO32- E) NO3

Give the correct number of electrons. A) eight B) one C) two D) five E) seven 24) in the second energy level of magnesium

fever of an infant weighing 8.5 pounds. The number of 37) A dose of aspirin of 5.0 mg per kilogram of body weight has been prescribed to reduce the milligrams of aspirin that should be administered is A) 19 mg B) 53 mg C) 1.6 mg D) 5.0 mg E) 0.59 mg

29) According to the atomic theory.. A) all atoms are different D) all matter is made up of tiny particles called electrons C) atoms of the same element combine to form compounds B) atoms are neither created nor destroyed during a chemical reaction E) a compound can contain different numbers of atoms as long as it has the same kinds of atoms

31) In an atom, the nucleus contains A) an equal number of protons and electrons B) all the protons and neutrons C) all the protons and electrons D) only neutrons E) only protons

35) 1 mole of a gas occupies 22.4 L at A) 0 °C and 0.50 atm B) 0°C and 760 mmHg C) 100 °C and 1 atm D) 100 °C and 10 atm E) OK and 1 atm

40) Double and triple bonds form because A) the atoms involved have high clectronegativities B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons C) one of the atoms in the molecule has more than 8 valence electrons D) the ions involved have charges larger than one E) there is at least one hydrogen atom involved in the bond.

Classify the following elements as metals, meralloids, or nonmetals A) metal B) nonmetal C) metalloid 17) chlorine

Classify the following elements as metals, metalloids, or nonmetals. A) metal B) nonmetal C) metalloid 16) phosphorus

Classify the following elements as metals, metalloids, or nonmetals. A) metal B) nonmetal C) metalloid 20) sulfur

Match the chemical name with the correct formula A) Mg(HSO4)2 B) MgSO4 C) MgS D) Mg(HSO3)2 E) MgSO3 15) magnesium sulfate

Match the statcl of matter with each of the following descriptions of a substance. A) liquid B) solid + liquid C) gas D) liquid + gas E) solid 5) This substance is melting.

Match the type of measurement to the unit given below. A) mass B) volume C) temperature D) length E) density 1) milliliter

16) A calcium atom two electrons in the fourth energy level.

True

16) As heat is removed from a solid, its temperature decreases

True

17) The formula of the compound chromium(III) oxide is Cr203.

True

11) How many equivalents are in 0.60 mole of Mg2+? A) 0.60 Eg B) 0.30 Eg C) 1.2 Eg D) 2.0 Eg E) 1.0 Eg

15) Which one of the following compounds contains an ion with a 3+ charge? A) KCL B) Nayo C) FeCl3 D) CUCI E) MgC2

16) The compound KOH is A) soluble, because all compounds containing OH- are soluble B) insoluble, because all compounds containing OH- are in soluble C) soluble, because all compounds containing K* are soluble D) insoluble, because all compounds containing K* are insoluble E) insoluble, because KOH is insoluble

17) An increase in the temperature of a solution usually A) increases the boiling point C) increases the solubility of a solid solute in the solution B) increases the solubility of a gas in the solution D) decreases the solubility of a solid solute in the solution E) decreases the solubility of a liquid solute in the solution

ml. How many milliliters of the suspension are required? 38) A doctor's order is 0.125 g of ampicillin. The liquid suspension on hand contains 250 mg/5.0 A) 0.0025 mL B) 3.0 ml C) 2.5 mL D) 6.3 ml. E) 0.0063 ml

46) The density of a solution is 1.18 g/mlIts specific gravity is A) 11.8 B) 0.118 C) 0.847 D) 1.18 E) 1.2

48) The maximum number of electrons that may occupy the third electron energy level is A) 2 B) 8 C) 10 D) 18 E) 32

59).If the heat of vaporization for water is 540 cal/g, how many kilocalories are released when 5.00 g of steam is converted to liquid at 100 C? A) 540 kcal B) 5.0 kcal C) 110 kcal D) 2.7 kcal E) 5.4 kcal

52) What element has the electron arrangement 2,8,4? A) carbon В) охудеn C) sulfur D) iron E) silicon

The heat of fusion of water is larger than the heat of vaporization.

False

Water freezes at 100 °C.

False

Write the symbol from the element name. 3) The symbol for mercury is

1) Air is an Example of a — mixture

Homogeneous

1) A sulfur atom gains electrons to form an ion with a charge of 2-.

True

10) 1 kg equivalent to 1000 mg.

True

10) The name of the compound CuQ is copper(II) oxide.

True

12) The name of the compound K3N is potassium nitride.

True

13) The formula for iron(II) sulfide is EeS.

True

14) The formula for hydroxide is OH-.

True

15) A lead atom with a mass number of 208 has 126 neutrons.

True

15) When A13+ and SO42- combine, the formula of the product is Al2(S04)3.

True

12) A gas has a volume of 36.0 L and a pressure of 750. torr when the temperature is 10. °C. What is the pressure if the volume changes to 15.0 L and the temperature changes to 78 °C, if the amount of gas stays the same?

2230 torr

Round off each of the following to three significant figures. 3) 25 225

25 200

Bramine (Brz) has a freezing point of -7 °C, and a boiling point of 60 °C. Indicate the state present or the change of state occurring at each temperature. 17) 60 °C

boiling or condensation

Identify each of the following compounds as covalent or ionic. 1) carbon tetrachloride

covalent

10) 200, mL of a 12.0% (m/v) NaCl solution is diluted to 600. ml. The new concentration is ——-%.

4.00 % (m/v)

Round off each of the following to three significant figures. 5) 399870

4.00 X 105

The specific heat of water (in /g "C) is

4.184 J/g °C

10) A food sample contains 6 g of carbohydrate and 4 g of protein. How many kcal from carbohydrate and protein are in the sample?

40 kcal

9) A gas has a pressure of 540. torg when the temperature is 127 °C. When the temperature changes to 27 °C, what is the new pressure, if there is no change in volume or amount of gas?

405 torr

14) What is the volume, in L, of 36.0 g of CH4 at STP?

50.3L

10) A gas has a pressure of 700. mmHg when the temperature is 107 °C. At what temperature (°C) will the pressure be 600. mmHg, if there is no change in volume or amount of gas?

53 °C

8) A temperature of 273 °C is equivalent to —K.

546 K

7) A gas has a volume of 46.0 L when the temperature is 400. K. When the termperature changes to 500. K, what is the new volume, if there is no change in pressure or amount of gas?

57.5 L

Round off each of the following to three significant figures. 6) 58.5422

58.5

9) A 2.0% (m/v) NACI solution contains ——-g NaCl in 300. mL of solution.

6.0 g

11) A solution which has 12 g of solute dissolved in 200.mL of solution has a m/v concentration of

6.0% (m/v)

Round off each of the following to three significant figures. 4) 6.3477 x 104

6.35 x 104

13) STP is —mmHg and —K.

760; 273

1) Nitrogen makes up about —percent of the atmosphere.

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