Chem Sum 19

How many liters of solution are there if the concentration of the solution is 1.8 M and there are a total of 0.50 moles of KCl dissolved? (A chance to use algebra! There is probably an example similar to this in my powerpoint.) A) 0.28 B) 0.21 C) 3.33 D) 0.56

A) 0.28

How many protons and neutrons are in this element: 195Pt? A) 78 protons, 117 neutrons B) 117 protons, 78 neutrons C) 78 protons, 195 neutrons D) 195 protons, 78 neutrons E) 195 protons, 117 neutrons

A) 78 protons, 117 neutrons

What order do electrons fill orbitals in the ground state? A) Electrons fill the lowest energy levels first. B) Electrons fill p orbitals first. C) Electrons fill the 3rd orbital first. D) Electrons enter the highest energy orbitals first. E) Electrons are placed four at a time in any orbital, starting in the s subshell.

A) Electrons fill the lowest energy levels first.

Which of the following best describe the charge and size of an electron?. A) Much smaller mass than a proton, but a much bigger electron "cloud" or area that it might be found. B) The same mass as a neutron but more negative charge. C) Half the mass of a proton, and the opposite charge. D) The electron cloud is smaller than the atomic nucleus, but more massive E) Electrons are so small that they don't exist.

A) Much smaller mass than a proton, but a much bigger electron "cloud" or area that it might be found.

Which bond will be hardest to break? A) N2 (a triple bond) B) O2 (a double bond) C) Cl2 (a single bond) D) F2 (a single bond)

A) N2 (a triple bond)

An atom that has more protons than electrons is A) a cation B) an anion C) a polyatomic ion D) a neutral atom

A) a cation

The sharing of two electrons between any two atoms in a compound is called _________. A) a covalent bond b) a formal attraction C) an intermolecular force D) the bond energy E) the electron affinity

A) a covalent bond

What kind of bond results when electron transfer occurs between atoms of two different elements? A) ionic B) covalent C) nonpolar D) single E) double

A) ionic

What does it mean when a molecule is said to be polar? A) one end of the molecule is slightly negative while the other end is slightly positive B) both ends of the molecule are slightly positive C) both ends of the molecule is slightly negative D) the molecule is neutral E) the difference in electronegativities is zero

A) one end of the molecule is slightly negative while the other end is slightly positive

How many protons and electrons are present in a S2- ion? A) 14 protons, 16 electrons B) 16 protons, 18 electrons C) 16 protons, 17 electrons D) 16 protons, 16 electrons E) 16 protons, 14 electrons

B) 16 protons, 18 electrons

A glucose solution with concentration 1.4 M fills a 2 liter flask exactly. How many moles of glucose would you ingest if you drank the entire 2 liter solution? A) 1.4 B) 2.8 C) 0.7 D) 5.6

B) 2.8

How many protons and electrons are present in a Ca2+ ion? A) 18 protons, 20 electrons B) 20 protons, 18 electrons C) 20 protons, 21 electrons D) 20 protons, 19 electrons E) 22 protons, 20 electrons

B) 20 protons, 18 electrons

What is the geometry for a molecule with 4 atoms bonded to the central atom (and no electron pairs on the central atom)? A) Linear B) Tetrahedral C) Trigonal planar D) Trigonal bipyramidal E) Octahedral

B) Tetrahedral

According to VSEPR theory, the shape of H2S would be __________. (Hint: find the Lewis dot structure. Hint about the hint: you can assume that S follows the octet rule)) (Another hint: It is very similar to water) A) linear B) bent / angular C) trigonal planar D) tetrahedral E) trigonal pyrimidal

B) bent / angular

Intermolecular forces are forces _______________. A) within molecules B) between molecules C) pushing molecules apart D) of attraction between the protons and electrons

B) between molecules

What is the quantity represented by the mass number minus the atomic number? A) number of atoms B) number of neutrons C) number of electrons D) number of protons E) number of particles in the nucleus

B) number of neutrons

Every atom of the same element has A) the same mass B) the same atomic number C) the same number of neutrons D) the same weight

B) the same atomic number

The maximum number of electrons that any p subshell can hold is A) 2 B) 4 C) 6 D) 10

C) 6

Which is the formula for a compound consisting of barium and fluoride? A) Ba2F3 B) BaF C) BaF2 D) Ba2F E) BaF3

C) BaF2

A neutralization reaction is one in which A) an acid neutralizes a base. B) a base neutralizes an acid. C) both A and B D) neither A nor B

C) Both a and b

Where are the halogens located on the periodic table? A) representative elements B) transition elements C) Group VIIA (17) D) Group IIA (2) E) Group IIIA (3)

C) Group VIIA (17)

The correct formula for the polyatomic ion, nitrate, is A) NO3 B) NO42- C) NO3- D) NO4 E) N-

C) NO3-

Which element matches the following electron configuration: 1s*2 2s*2 2p*6 3s*2 3p*6 4s*2 A) potassium B) sodium C) calcium D) magnesium

C) calcium

Assuming reactions between the following pairs of elements, which pair is most likely to form an ionic compound? A) copper and tin B) chlorine and oxygen C) cesium and iodine D) carbon and chlorine E) fluorine and iodine

C) cesium and iodine

What type of change happens during the decay of a fallen tree, as compounds in the wood are changed to new ones with the help of microorganisms? A) intensive B) extensive C) chemical D) physical E) potential

C) chemical

Which of the following is NOT a physical property of matter? A) odor B) compressibility C) flammability D) color E) melting point

C) flammability

An element in the periodic table will have more similar properties to other elements in the same ____________ . A) row B) isotope C) group D) molecule E) density

C) group

Air is mostly nitrogen, a lot of oxygen, and some argon, carbon dioxide (CO2), water vapor (H2O) and a few other things. Therefore, air is a/an: A) element. B) compound. C) mixture. D) molecule. E) pure substance.

C) mixture.

Identify this element: 133 X 55 Cs Ba Xe As B

Cs

Which one of the following is the most polar bond? (Hint: think about the electronegativities of the atoms involved) A) B - C B) S - O C) N - O D) B - O E) C - C

D) B - O

Which of the following reagents is not a strong acid or strong base? A) HNO3 B) NaOH C) HCl D) CH3COOH E) H2SO4

D) CH3COOH

Which element has the greatest electronegativity? A) C B) Si C) As D) Cl E) Sr

D) Cl

The melting of saltwater (with all the salt always dissolved) is A) a chemical change of a homogenous mixture B) a physical change of a heterogenous mixture C) a chemical change of a heterogenous mixture D) a physical change of a homogenous mixture E) none of the above

D) a physical change of a homogenous mixture

Water has a ____________ shape while carbon dioxide has a __________ shape because water has __________. A) bent/angular, tetrahedral, hydrogen bonds B) linear, linear, 2 hydrogens C) linear, trigonal planar, 2 non-bonding electron pairs D) bent/angular, linear, 2 non-bonding electron pairs E) tetrahedral, linear, electronegativity

D) bent/angular, linear, 2 non-bonding electron pairs

Valence electrons are A) electrons that are not involved in bonding. B) the total number of electrons in an atom. C) electrons in the innermost shell of an atom. D) electrons in the outermost shell of an atom.

D) electrons in the outermost shell of an atom.

What is the name of SO3? A) sulfur oxygen B) sulfite C) sulfate D) sulfur trioxide

D) sulfur trioxide

According to VSEPR theory, if the valence electrons on a central atom are 3 bound pairs and one non-bonding (lone) pair, the geometry (shape) at this atom will be ______________. A) linear B) bent (angular) C) trigonal planar D) trigonal pyramidal E) tetrahedral

D) trigonal pyramidal

How many bonding electrons are in CO2? A) 1 B) 2 C) 3 D) 4 E) 8

E) 8

Which one of the following elements has the highest electron affinity? A) Li B) K C) Kr D) O E) Cl

E) Cl

What is the name given to atoms of an element having a different number of electrons than protons? A) Cations B) Anions C) Protons D) Isotopes E) Ions

E) Ions

What kind of change always results in the formation of new materials/substances? A) molecular B) exothermic C) endothermic d) physical E) chemical

E) chemical

A double bond between two atoms, A and B _____________. A) is longer than a single bond between the same two atoms B) has a lower bond energy than a single bond between the same two atoms C) arises when two electrons are transferred from a to b D) consists of two electrons shared between a and b E) consists of four electrons shared between a and b

E) consists of four electrons shared between a and b

What is the shape of a p orbital? A) tetrahedral B) sphere C) 4 leaf clover shape D) two lobes and a donut E) figure 8 or infinity sign / 3 dimensional dumbell F) too complicated

E) figure 8 or infinity sign / 3 dimensional dumbell

According to the Aufbau principle, the orbitals that electrons will occupy first will be A) those in the p subshell B) The ones with electron density farthest from the nucleus C) the highest energy orbitals D) those in the d subshell E) the lowest energy orbitals

E) the lowest energy orbitals

According the periodic table or the diagonal electron filling diagram, the 4s subshell is filled before the 3d subshell. A) True B) False

True

Atoms of the noble gas elements, Group VIII A (18), do not usually form bonds with any other elements. True False

True

In the scientific method, a theory can be trusted to be true more than a hypothesis can. True False

True

The two strands of double stranded DNA are held together by hydrogen bonds. True False

True

One balloon contains 1.5 moles of hydrogen (molar mass of 2 g/mole). Another balloon contains 1 mole of nitrogen (28 g/mole). A third contains 0.5 moles oxygen (32 g/mole). At the same same temperature and pressure, what do we know about the sizes of the balloons? a. The hydrogen balloon is bigger in volume b. The nitrogen balloon is bigger in volume. c. The will all be within 5% of being the same volume. d. There is not enough information to know how their volumes will compare. e. The oxygen balloon is bigger in volume.

a. The hydrogen balloon is bigger in volume

Which element has an atomic number of 3 and mass number of 7? a. 7 Li b.4 Li c. 10 Ne d. 10 N e. 7 Be

a. 7 Li

Which of the following is both a quantitative and a qualitative statement? a. The reaction produced 112 g of a pure white solid. b. The compound has a mass of 14.62 g. c. The compound formed pale yellow crystals. d. The drug is 92.5% pure. e. The compound melted.

a. The reaction produced 112 g of a pure white solid.

Which of the following describes a chemical change? a. fermenting wine b. boiling water c. grinding coffee beans d. crushing an aluminum can e. bending copper wire

a. fermenting wine

The term "hydrophobic" means which of the following? a. water-hating b. water-soluble c. water-attracting d. water-loving e. water-hating and water-soluble

a. water-hating

10. What is the oxidation number of N in NH4+ ? a. −3 b. −1 c. 0 d. +1 e. +3

a. −3

If, at constant pressure, the absolute temperature of a flask equipped with a moveable piston is reduced to half its original absolute temperature, what must be the new volume?a. 1/4 the original volume b. 1/2 the original volume c. two times the original volume d. four times the original volume e. equal to the original volume

b. 1/2 the original volume

Arrange the following gaseous substances in order of decreasing average molecular speed at 25°C: argon, fluorine, carbon dioxide, oxygen, helium (hint: what characteristic of the gas is important here? hint2: there is a relevant graph in the presentation slides) a. helium > oxygen > fluorine > carbon dioxide > argon b. helium > oxygen > fluorine > argon > carbon dioxide c. argon > oxygen > helium > carbon dioxide > fluorine d. carbon dioxide > argon > fluorine > oxygen > helium e. carbon dioxide > fluorine > argon > oxygen > helium

b. helium > oxygen > fluorine > argon > carbon dioxide

There are _____ milligrams in a kilogram. a. 1 ´ 10*-3 b. 1 ´ 10*6 c. 1 ´ 10*9 d. 1 ´ 10*-6 e. 1 ´ 10*3

b. 1 ´ 10*6

How many moles of NaOH are present in 25.0 mL of a 0.1000 M NaOH solution? a. 100 mol b. 2.50 ⋅ 10−3 mol c. 0.100 mol d. 2.50 mol e. 25.0 mol

b. 2.50 ⋅ 10−3 mol

Converting 6.390 pounds to grams yields: a. 2516 g. b. 2898 g. c. 6390 g. d. 14090 g. e. 16230 g.

b. 2898 g.

Which of the following statements concerning the atom is false? a. The radius of an atom is approximately 10,000 times larger than the radius of the nucleus. b. A neutral atom sometimes has different numbers of protons and electrons. c. Electrons are found in orbits about the nucleus. d. The nucleus contains both protons and neutrons. e. Most of the mass of the atom is found in the nucleus.

b. A neutral atom sometimes has different numbers of protons and electrons.

Which one of the following does not have the electron configuration [Ne]3s*2 3p*6? a.Ar b. Br− c. Ca2+ d. Cl− e. K+

b. Br−

Which statement about light is true? a. It oscillates back and forth between wave and particle-like behavior. b. It exhibits both wave and particle-like behavior at the same time. c. It has neither wave nor particle-like behavior. d. It behaves as a particle only. e. It behaves as a wave only.

b. It exhibits both wave and particle-like behavior at the same time.

Which statement regarding an orbital is false? a. An orbital is three dimensional. b. Only one electron is allowed per orbital. c. An electron shell consists of a collection of orbitals with the same principal quantum number. d. Any electrons in a specific orbital must have the same principle quantum number. e. An orbital boundary surface would need to be infinitely large to guarantee that an electron would always be found inside the orbital.

b. Only one electron is allowed per orbital.

A sample has a mass of 612 g and a volume of 78 cm3. What is the identity of the sample? a. mercury (density = 13.6 g/cm3) b. iron (density = 7.86 g/cm3) c. copper (density = 8.92 g/cm3) d. silver (density = 10.5 g/cm3) e. aluminum (density = 2.7 g/cm3)

b. iron (density = 7.86 g/cm3)

Which one of the following correctly lists the relative strengths of electron-pair repulsions? a. bonding pair-bonding pair > lone pair-bonding pair > lone pair-lone pair b. lone pair-lone pair > lone pair-bonding pair > bonding pair-bonding pair c. lone pair-lone pair > bonding pair-bonding pair > lone pair-bonding pair d. lone pair-bonding pair > lone pair-lone pair > bonding pair-bonding pair e. bonding pair-bonding pair > lone pair-lone pair > lone pair-bonding pair

b. lone pair-lone pair > lone pair-bonding pair > bonding pair-bonding pair

If heat is transferred from the system to the surroundings then a. q system is positive b. q system is negative c. the system is doing work d. the surroundings are doing work e. Both q system is positive and the system is doing work.

b. q system is negative

Which statement is false? a. Atmospheric gases are an example of gases mixing completely. b. An exhaled breath of air will disperse throughout the entire atmosphere. c. A gas inside a container will remain inside indefinitely if the container is opened. d. Atmospheric pressure is a result of gas molecules exerting pressure on their surroundings. e. An air pump demonstrates that gases can be compressed.

c. A gas inside a container will remain inside indefinitely if the container is opened.

Data show a strong correlation between atmospheric carbon dioxide levels and global temperature. There is a strong scientific consensus that this is a causal relationship. What is an explanation to support the hypothesis that carbon dioxide causes an increase in Earth's temperature? a. carbon dioxide acts as a blanket and insulates the Earth b. carbon dioxide molecules are able to store a high amount of energy that they acquire in the daytime. c. CO2 molecules absorb IR (infrared radiation) that comes from the Earth and would otherwise escape d. CO2 reacts exothermically with argon in the atmosphere and gives off a lot of heat. e. all of these choices

c. CO2 molecules absorb IR (infrared radiation) that comes from the Earth and would otherwise escape

When the external pressure on a balloon is decreased at constant temperature, what happens to the gas inside? a. The collisions become more elastic. b. The gas undergoes no changes. c. The volume increases. d. The molecules increase in rate of movement. e. The volume decreases.

c. The volume increases.

For a gas mixture a. the partial pressures of the gases at equilibrium are equal. b. the total pressure is equal to the maximum partial pressure. c. the total pressure is equal to the sum of the partial pressures. d. the lightest gas will have the lowest partial pressure. e. the lightest gas will have the highest partial pressure.

c. the total pressure is equal to the sum of the partial pressures.

Permanent magnets are: a. paramagnetic. b. diamagnetic. c. ferromagnetic. d. lanthanides. e. isoelectronic.

c. ferromagnetic.

How many of each types of atoms does the compound mercury acetate, Hg2(C2H3O2)2 contain? a. 2 mercury, 2 carbon, 3 hydrogen, 2 oxygen b. 4 mercury, 4 carbon, 6 hydrogen, 4 oxygen c. 2 mercury, 4 carbon, 6 hydrogen, 4 oxygen d. 1 mercury, 2 carbon, 3 hydrogen, 2 oxygen e. 2 mercury, 2 carbon, 3 hydrogen, 4 oxygen

c. 2 mercury, 4 carbon, 6 hydrogen, 4 oxygen

What will take the most energy? (Constants: Heat of fusion of water: 334 J/g Heat of vaporization of water: 2260 J/g Specific heat capacity of copper: 0.385 J/g*C Specific heat capacity of gold: 0.129 J/g*C Specific heat capacity of water: 4.18 J/g*C) a. Increase the temperature of 10 grams of solid gold by 15 degrees b. Increase the temperature of 10 grams of solid water (ice) by 12 degrees c. Evaporate 10 grams of water d. Increase the temperature of 10 grams of copper by 15 degrees. e. Freeze 10 grams of water.

c. Evaporate 10 grams of water

Which of the following represents a pair of allotropes? a. air and oxygen b. glucose and sucrose c. graphite and diamond d. sand and glass e. carbon monoxide and carbon dioxide

c. graphite and diamond

Which azimuthal quantum numbers can exist for n = 3? a. l = 0 b. l = 0, 1 c. l = 0, 1, 2 d. l = 0, 1, 2, 3 e. l = 0, 1, 2, 3, 4

c. l = 0, 1, 2

Which of the following central atoms would be expected to accommodate more than four electron pairs in some of its compounds? a. fluorine b. boron c. sulfur d. carbon e. helium

c. sulfur

How many significant figures are present in each of the following: 86.9, 3.710, and 0.0492? a. three, three, three b. three, three, four c. three, four, three d. three, four, four e. three, four, five

c. three, four, three

Clean air a. is pure oxygen. b. contains mostly oxygen, some nitrogen and nothing else. c. contains mostly nitrogen, some oxygen and nothing else. d. contains mostly nitrogen, some oxygen, and a very small amount of several other gases. e. has all of its nitrogen removed.

d. contains mostly nitrogen, some oxygen, and a very small amount of several other gases.

How many total valence electrons will be in the correctly drawn Lewis Structure for CHCl3? a. 8 b. 16 c. 24 d. 26 e. 32

d. 26

Which of the following statements is/are correct? I. The frequency of light is the number of waves that pass a given point in a second. II. The shorter the wavelength of light, the greater its energy. III. The wavelength of light increases as the frequency increases. a. I only b. II only c. III only d. I and II e. II and III

d. I and II

Which of the following statements is/are correct? I. The frequency of light is the number of waves that pass a given point in a second. II. The shorter the wavelength of light, the greater its energy. III. The wavelength of light increases as the frequency increases. a. I only b. II only c. III only d. I and II e. II and III

d. I and II

Three elements that are likely to have similar chemical and physical properties are: a. B, K, U b. Ca, Co, Cr c. B, Br, Bi d. Mg, Ca, Ba e. Al, Si, P

d. Mg, Ca, Ba

A "free radical" is which of the following? a. formed from the combination of two photons b. a negatively charged species c. a species that exists only in theory, not in reality d. an atom or a molecule containing an unpaired electron e. very stable and unreactive

d. an atom or a molecule containing an unpaired electron

Which of the following correctly describes the relationship between the pressure of a gas and the volume of a gas at constant temperature? a. as one increases the other increases b. unrelated c. directly proportional d. irreversibly proportional e. inversely proportional

e. inversely proportional

Which of the following corresponds to the electron configuration of a noble gas? a. 1s*2 2s*2 b. 1s*2 2s*2 2p*4 c. 1s*2 2s*2 2p*6 3s*2 3p*6 3d*10 4s*2 4p*2 d. 1s*2 2s*2 2p*6 3s*2 3p*6 3d*10 4s*2 4p*3 e. 1s*2 2s*2 2p*6 3s*2 3p*6

e. 1s*2 2s*2 2p*6 3s*2 3p*6

A photon of light has a frequency of 3.26 ⋅1015 hertz. What is its wavelength? The speed of light is 3.00 ⋅ 108 m/s. a. 1.09 ⋅ 107 nm b. 9.78 ⋅ 1014 nm c. 978 nm d. 109 nm e. 92.0 nm

e. 92.0 nm

Which compound is not a hydrocarbon? a. C2H6 b. C2H2 c. C6H14 d. CH4 e. CH3OH

e. CH3OH

Select the element which never forms more than one bond in a Lewis Dot structure. a. O b. C c. N d. Al e. H

e. H

Which characteristics apply to the gaseous state? I. low density II. high density III. rapid molecular motion IV. slow molecular motion V. large distance between particles a. I, V b. II, V c. II, III, V d. I, IV, V e. I, III, V

e. I, III, V

Which element has a small first ionization energy, and very large second and third ionization energies? a. Mg b. Al c. S d. Ar e. K

e. K

Which one of the following does not have the electron configuration [Ne]3s23p6? a. Ar b. Br− c. Ca2+ d. Cl− e. K+

e. K+

In Rutherford's gold foil experiment: a. Electrons passed straight through gold foil. b. Rutherford's expectations for the experiment were proven to be correct. c. Neutrons were discovered. d. Helium ions collided with each other e. Rutherford concluded that there must be a compact concentration of positive charge inside the gold atoms.

e. Rutherford concluded that there must be a compact concentration of positive charge inside the gold atoms.

Give the formula for the ionic compound that forms between strontium and fluorine. a. Sr2F b. Sr2F3 c. Sr2F4 d. SrF e. SrF2

e. SrF2

Arrange the following four electromagnetic spectral regions in order of decreasing energy. visible X-ray microwave radio a. microwave, radio, X-ray, visible b. microwave, visible, X-ray, radio c. radio, visible, X-ray, microwave d. X-ray, radio, visible, microwave e. X-ray, visible, microwave, radio

e. X-ray, visible, microwave, radio

Which atom(s) is (are) not found in an alkane or any hydrocarbon? a. all halogens b. noble gasses c. P, N, O d. P, S, Br, Al e. all of the above

e. all of the above

Which of the following is a greenhouse gas? a. carbon dioxide b. methane c. ozone d. water vapor e. all of these choices

e. all of these choices

Which characteristic below best fits the description of a solid? a. large distances between the molecules b. molecules that are close together but are moving past one another c. highly disordered molecules d. rapid molecular motion e. highly ordered molecules

e. highly ordered molecules

Which word or phrase least applies to the quantum number represented by the symbol n? a. shell b. size c. principal d. distance from nucleus e. shape

e. shape

According the periodic table or the diagonal electron filling diagram, the 4s subshell is filled before the 3d subshell. True False

true