Chemistry Chapter 4 study
(A) Protons and neutrons have a mass of ______. (B) Electrons, essentially, have a mass of ______. (C) The nucleus of atom is about _______ the size of an electron. (D) The entire atom is about _______ the size of the nucleus.
(A). 1 (B). 0 (C). 2000 times (D). 40000 times
Thomson proposed a (A)________ with (B)______ particles embedded on the outer surface. What is the model called?
(A).Positive Ball (B).Negative Called the Plum Pudding Model
All atoms of one element are (A)________, but they (B)___________ from atoms of other elements.
(A)Identical (B)Different
What Japanese Physicist, (A)_______, and (B)______ both proposed electrons (C)____________, like a moon around a planet.
(A)Nagaoka (B)Neils Bohr (C)Orbit a positive nucleus
Early Greek Philosophers (600 B.C.): Thought about matter, proposed that all things were made of 4 _______: ________ , _________, _________, and __________.
(In order as they appear) Element; Earth; Wind; Fire; Air
21 cm is the same distance as a. 0.0521 m. b. 52.1 dm. c. 5.21 mm. d. 0.00521 km. e. 5210 m.
0.0521 m.
What is the correct answer for the calculation of a volume (in mL) with measured numbers ? a. 0.22 mL b. 0.223 mL c. 57 mL d. 14 mL e. 14.3 mL
0.22 mL
What is the metric relationship between grams and micrograms? a. 1 g = 100 μg b. 1 g = 1 000 000 μg c. 1 g = 0.000 001 μg d. 1 g = 1000 μg e. 1 g = 0.001 μg
1 g = 1 000 000 μg
A 50.0 mL urine sample has a mass of 50.7 g. The specific gravity of the urine is a. 1.014 g/mL. b. 0.986 g/L. c. 1.01. d. 0.986. e. 50.7.
1.01
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
1.33 g/mL
One atomic mass unit is equal to what?
1/12 the mass of a Carbon-12 Atom
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.
100 g of water by 10 °C.
The dietary calorie(Cal) is equal to a. 1000 kilocalories. b. 1000 calories. c. 100 calories. d. 10 calories. e. 1 calorie.
1000 calories
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
101.3 °F
____ 100. 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
11
The number of calories needed to raise the temperature of 32 g of water from 12 °C to 54 °C is 380 cal. b. 1.3 cal. c. 1300 cal. d. 1700 cal. e. 0.76 cal.
1300 cal
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. 13.6 J
13600 J
The correct answer for the addition of 7.5 g + 2.26 g + 1.311 g + 2 g is 13.071 g. b. 13 g. c. 13.0 g. d. 10 g. e. 13.1 g.
13g
How many centimeters are there in 57.0 in.? a. 22 cm b. 0.0445 cm c. 145 cm d. 22.4 cm e. 140 cm
145 cm
650. J is the same amount of energy as ________. a. 155 cal b. 2720 cal c. 650. cal d. 1550 cal e. 2.72 cal
155 cal
Which of the following numbers contains the designated correct number of significant figures? a. 0.04300 5 significant figures b. 0.00302 2 significant figures c. 156 000 3 significant figures d. 1.04 2 significant figures e. 3.0650 4 significant figures
156 000 - 3 SigFigs
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
1600 cal
How many protons are in Cl-52?
17
The maximum number of electrons that may occupy the third electron energy level is a. 2. b. 8. c. 10. d. 18. e. 32.
18
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
19.3 mL
All isotopes of Helium contain ________.
2 Protons
What is the correct electron arrangement for the lithium atom? a. 3 b. 3,1 c. 1,2 d. 2,1 e. 2,5
2, 1
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
2, 8, 3
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
2, 8, 8, 1
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
2.30 kg
A doctor's order is 0.125 g of ampicillin. The liquid suspension on hand contains 250 mg/5.0 mL. How many milliliters of the suspension are required? a. 0.0025 mL b. 3.0 mL c. 2.5 mL d. 6.3 mL e. 0.0063 mL
2.5 mL
What is the density of a substance with a mass of 45.00 g and a volume of 26.4 mL? a. 1.70 g/mL b. 1.7 g/mL c. 0.59 g/mL d. 0.587 g/mL e. 45.0 g/mL
2.70 g/mL
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
2.7kcal
Which of the following examples illustrates a number that is correctly rounded to three significant figures? a. 4.05438 grams to 4.054 grams b. 0.03954 grams to 0.040 grams c. 103.692 grams to 103.7 grams d. 109 526 grams to 109 500 grams e. 20.0332 grams to 20.0 grams
20.0332 grams to 20.0 grams
Which of the answers for the following conversions contains the correct number of significant figures? a. 2.543 m x 39.4 in/1m = 100.1942 in b. 2 L x 1.06qt/1L = 2.12 qt c. 24.95 min x 1hr/60min = 0.4158 hr d. 12.0 ft x 12in/1ft x 2.54cm/1in = 370 cm e. 24.0 kg x 1lb/2.20kg = 11 lb
24.95 min x 1hr/60min = 0.4158 hr
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
240 kcal
Which of the following conversion factors is a measured number? a. 10 cm/dm b. 12 in/ft c. 16 oz/lb d. 25 miles/gallon e. 12 eggs/dozen
25 miles/gallon
What is 6.5 m converted to inches? a. 1700 in b. 1651 in c. 39 in d. 260 in e. 255.9 in
260 in
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
2800 cal
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
3
The number of electron energy levels in a magnesium atom is a. 1. b. 2. c. 3. d. 4. e. 5.
3
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.
3
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
3.6 x 103 cal
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.
30
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 kcal d. 630 kcal e. 280 kcal
360 kcal
What is the mass number of an atom of potassium that has 20 neutrons? a. 15 b. 19 c. 35 d. 39 e. 59
39
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 cm3 b. 4.29 cm3 c. 0.233 cm3 d. 53 cm3 e. 53.2 cm3
4.29 cm3
The measurement 0.000 004 3 m, expressed correctly using scientific notation, is 4.3 x 10-7 m. b. 4.3 x 10-6 m. c. 4.3 x 106 m. d. 0.43 x 10-5 m. e. 4.3 m.
4.3 x 10-6 m.
The number of neutrons in Ga-71 is what?
40
The EPA limit for lead in the soil of play areas is 400 ppm. This is the same as a. 400 mg lead in each gram of soil. b. 400 g lead in each kilogram of soil. c. 400 mg lead in each kilogram of soil. d. 400 µg lead in each kilogram of soil. e. 400 µg lead in each milligram of soil.
400 mg lead in each gram of soil.
The correct symbol for the isotope of potassium with 22 neutrons is a. 41/19K b. 19/41K c. 37/15K d. 15/37K e. 22/19K
41/19K
A calculator answer of 423.6059 must be rounded off to three significant figures. What answer is reported? a. 423 b. 424 c. 1.7420 d. 423.6 e. 423.7
424
1.00 pint of milk has a volume of how many milliliters? (2 pints = 1 quart) a. 472 mL b. 530. mL c. 1000 mL d. 1890 mL e. 106 mL
472 mL
A temperature of 41 °F is the same as a. 5 °C. b. 310 °C. c. -9 °C. d. 16 °C. e. 42 °C.
5 °C
Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of ? 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
50 protons, 68 neutrons, 50 electrons
What is the number of neutrons in Ga-89
58 Neutrons in Ga-89
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.
64
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
68 °F
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
693 cal
How many pounds are in 3.5 kg? a. 7.7 lb b. 1.59 lb c. 0.629 lb d. 1.6 lb e. 7.70 lb
7.7 lb
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
77 K
Which of the following measurements are not equivalent? a. 25 mg = 0.025 g b. 183 L = 0.183 kL c. 150 ms = 0.150 s d. 84 cm = 8.4 mm e. 24 dL = 2.4 L
84 cm = 8.4 mm
How many calories are required to increase the temperature of 13 g of alcohol from 11 °C to 23 °C? The specific heat of alcohol is 0.59 cal/g °C. a. 83 cal b. 0.63 cal c. 92 cal d. 0.54 cal e. 170 cal
92 cal
9.31 g is the same mass as 931 μg. b. 931 kg. c. 93.1 cg. d. 9310 mg. e. 0.0931 dg.
9310 mg
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.
A proton has a positive charge and a mass of approximately 1 amu.
Dalton's Atomic Theory includes which idea? A. Atoms of the same element are always identical. B. Atoms of different elements always combine in one-to-one ratios. C. All atoms of all elements are the same size. D. Individual atoms can be seen with a microscope.
A. Atoms of the same element are always identical.
An atom has 52 electrons, a neutral charge, and 85 neutrons, which of the following is the correct chemical symbol for for this. A.Te-137 B.Te-85 C.Ga-137 D.Au-52
A. Te has 52 protons and electrons, and 85 neutrons plus 52 electrons=137. Making your answer Te-137
What units is the atomic mass unit reported in?
AMU
The sybol for aluminum is: a. Al b. Am c. Au d. Sn e. Ag
Al
What is the name of the particle Rutherford used in his experiment?
Alpha Particle
What kind of particle did Rutherford fire at the gold foil in his experiment? What was their charge?
Alpha Particles, Charge 2+
Radiation deflected towards the negatively charged plate.
Alpha Radiation
Who observed that systems always had the same mass before and after a reaction, and called this observation the Law of Conservation of Mass
Antione Lavosier (1782)
Which of the following elements is a noble gas? a. oxygen b. chlorine c. bromine d. argon e. nitrogen
Argon
The smallest particle of an element that retains the properties of that element.
Atom
What element of chemistry is comprised of three units (proton, neutron, electron)?
Atom
What is an equation showing the relationship between an atom's atomic number and its mass number.
Atomic # + Neutrons = Mass #
The weighted average mass of an element's isotopes.
Atomic Mass
Equal to 1/12 the mass of a Carbon-12 Atom.
Atomic Mass Unit
The number of protons in an atom, identifies it as a certain element.
Atomic Number
All atoms of the same element have the same what?
Atomic Number (this is the number of protons in an element, if the number of protons change in the atom, it turns into a new element.)
Because most particles fired at metal foil passed straight through, Rutherford concluded what?
Atoms were mostly empty space.
What of the following Isotopes has the same number of electrons? A. Au-197 B.Li-7 C.Li-127 D.Mg-25
B & C (They are the same element, and they have a neutral charge, so they have the same number of electrons)
Today scientist believe that an atom is the ____ ____ _____.
Basic Chemical Unit
Radiation deflected toward the positively charge plate.
Beta Radiation
Which element would have physical and chemical properties similar to chlorine? a. Ar b. Br c. S d. O e. P
Br
The rays and particles emitted by radioactive material.
Cathode Ray
The deflection of the cathode rays in Thomson's experiments was evidence of the _____ nature of electrons.
Charged
What is the element with the electron arrangement 2,8,7? a. Be b. Cl c. F d. S e. Ar
Cl
The scientist who is credited with the invention of the cathode ray tube is?
Crookes
states that all matter is composed of atom's.
Dalton's Atomic Theory
Who proposed that the world is made of empty space and tiny particles called atomos?
Democrates (460-370 B.C.)
Thomson then, as he was studying electrons and protons discovered that some elements (neon) have atoms of ________. Now called isotopes.
Different masses
Most of the volume of an atom is made up by the ______.
Electron Cloud
Where in the atom is the electron found?
Electron Cloud
True or False: Ancient philosophers regularly performed controlled experiments.
False
True or False:An alpha particle consists of two protons and two electrons.
False
True or False:An atom's nucleus contains its protons and electrons.
False
True or False:Beta Particles have a charge of 2+.
False
True or False:Dalton was correct in thinking that atoms could not be divided into smaller particles.
False
True or False:Dalton's atomic theory stated that matter is mostly empty space.
False
True or False:Democritus proposed that atoms are held together by chemical bonds, but no one believed him.
False
True or False:Most atoms have either a positive or negative charge.
False
True or False:The nucleus takes up most of the volume of the atom.
False
True or False:The number of neutrons in an atom is referred to as its atomic number.
False
High-energy radiation that has no charge and no mass.
Gamma Ray
Atoms with the same number of protons but different number of neutrons.
Isotopes
The mass of a neutron is about equal to what?
Its about the same as the mass of a proton.
Who discovered the electron in 1897?
J.J. Thomson
Who compiled the work of previous scientists and came up with the Atomic Theory?
John Dalton (1803)
Who observed that water is always 11% hydrogen and 89% Oxygen by mass. Now called the Law of Definite Proportions.
Joseph Prust (1799)
What scientist is credited with the Law of Conservation of Mass?
Lavoisier
Which of the following is not a chemical? a. salt b. water c. light d. carbon dioxide e. sugar
Light
Titanium dioxide is a chemical used in toothpaste to ________. a. make the paste white b. disinfect the toothbrush c. keep the paste from spoiling d. remove plaque e. strengthen tooth enamel
Make paste White
The ______ of this particle, named a proton, was found to be much higher than that of the electron.
Mass
The atomic mass of an element depends upon the _______.
Mass and Relative Abundance of each isotope of that element.
The number of protons and neutron in the nucleus of an atoms is what?
Mass number
Aluminum (Al)
Metal
Bismuth (Bi)
Metal
Gallium (Ga)
Metal
Indium (In)
Metal
Lead (Pb)
Metal
Polonium (Po)
Metal
Thallium (Tl)
Metal
Tin (Sn)
Metal
Actinum (Ac)
Metal Actinide
Americium (Am)
Metal Actinide
Berkelium (Bk)
Metal Actinide
Californium (Cf)
Metal Actinide
Curium (Cm)
Metal Actinide
Einsteinium (Es)
Metal Actinide
Fermium (Fm)
Metal Actinide
Lawrencium (Lr)
Metal Actinide
Mendelevium (Md)
Metal Actinide
Neptunium (Np)
Metal Actinide
Nobelium (No)
Metal Actinide
Plutonium (Pu)
Metal Actinide
Protactinium (Pa)
Metal Actinide
Thorium (Th)
Metal Actinide
Uranium (U)
Metal Actinide
Cesium (Cs)
Metal Alkali Metal
Francium (Fr)
Metal Alkali Metal
Lithium (Li)
Metal Alkali Metal
Potassium (K)
Metal Alkali Metal
Rubidium (Rb)
Metal Alkali Metal
Sodium (Na)
Metal Alkali Metal
Barium (Ba)
Metal Alkaline Metal
Beryllium (Be)
Metal Alkaline Metal
Calcium (Ca)
Metal Alkaline Metal
Magnesium (Mg)
Metal Alkaline Metal
Radium (Ra)
Metal Alkaline Metal
Strontium (Sr)
Metal Alkaline Metal
Cerium (Ce)
Metal Lanthanide
Dysprosium (Dy)
Metal Lanthanide
Erbium (Er)
Metal Lanthanide
Europium (Eu)
Metal Lanthanide
Gadolinium (Gd)
Metal Lanthanide
Holmium (Ho)
Metal Lanthanide
Lanthanum (La)
Metal Lanthanide
Lutetium (Lu)
Metal Lanthanide
Neodymium (Nd)
Metal Lanthanide
Praseodynium (Pr)
Metal Lanthanide
Promethium (Pm)
Metal Lanthanide
Samarium (Sm)
Metal Lanthanide
Terbium (Tb)
Metal Lanthanide
Thulium (Tm)
Metal Lanthanide
Ytterbium (Yb)
Metal Lanthanide
Bohrium (Bh)
Metal Transition Metal
Cadmium (Cd)
Metal Transition Metal
Chronium (Cr)
Metal Transition Metal
Cobalt (Co)
Metal Transition Metal
Copernicium (Cn)
Metal Transition Metal
Copper (Cu)
Metal Transition Metal
Darmstadtium (Ds)
Metal Transition Metal
Dubnium (Db)
Metal Transition Metal
Gold (Au)
Metal Transition Metal
Hafnium (Hf)
Metal Transition Metal
Hassium (Hs)
Metal Transition Metal
Iridium (Ir)
Metal Transition Metal
Iron (Fe)
Metal Transition Metal
Manganese (Mn)
Metal Transition Metal
Meitmerium (Mt)
Metal Transition Metal
Mercury (Hg)
Metal Transition Metal
Molybdenum (Mo)
Metal Transition Metal
Nickel (Ni)
Metal Transition Metal
Niobium (Nb)
Metal Transition Metal
Osmium (Os)
Metal Transition Metal
Palladium (Pd)
Metal Transition Metal
Platinum (Pt)
Metal Transition Metal
Rhenium (Re)
Metal Transition Metal
Rhodium (Rh)
Metal Transition Metal
Roentgenium (Rg)
Metal Transition Metal
Ruthenium (Ru)
Metal Transition Metal
Rutherfordium (Rf)
Metal Transition Metal
Scandium (Sc)
Metal Transition Metal
Seaborgium (Sg)
Metal Transition Metal
Silver (Ag)
Metal Transition Metal
Tantalum (Ta)
Metal Transition Metal
Technetium (Tc)
Metal Transition Metal
Titanium (Ti)
Metal Transition Metal
Tungsten (W)
Metal Transition Metal
Vandium (V)
Metal Transition Metal
Yttrium (Y)
Metal Transition Metal
Zinc (Zn)
Metal Transition Metal
Zirconium (Zr)
Metal Transition Metal
Antimony (Sb)
Metalloid
Arsenic (As)
Metalloid
Boron (B)
Metalloid
Germanium (Ge)
Metalloid
Silicon (Si)
Metalloid
Tellurium (Te)
Metalloid
Astratine (At)
Metalloid Halogen
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.
Most of them are liquids at room temperature.
The existence of ________, this third neutral particle, was confirmed in 1930 by who?
Neutron, discovered by Chadwick.
Isotopes of the same element have different what?
Neutrons
What happens to an atom when you add a proton?
New element is formed.
What happens to an atom when you add a neutron?
New isotope is formed.
Carbon (C)
Nonmetal
Hydrogen (H)
Nonmetal
Nitrogen (N)
Nonmetal
Oxygen (O)
Nonmetal
Phosphorous (P)
Nonmetal
Selenium (Se)
Nonmetal
Sulfur (S)
Nonmetal
Bromine (Br)
Nonmetal Halogen
Chlorine (Cl)
Nonmetal Halogen
Fluorine (F)
Nonmetal Halogen
Iodine (I)
Nonmetal Halogen
Argon (Ar)
Nonmetal Noble Gas
Helium (He)
Nonmetal Noble Gas
Krypton (Kr)
Nonmetal Noble Gas
Neon (Ne)
Nonmetal Noble Gas
Radon (Rn)
Nonmetal Noble Gas
Xenon (Xe)
Nonmetal Noble Gas
The center-most part of an atom where the protons and neutrons.
Nucleus
What atomic structure did Rutherford discover in his experiment?
Nucleus
Where in the atoms is the proton found?
Nucleus
The production of smog from NO gas requires ________. a. nitrogen b. chlorine c. water d. oxygen e. CFCs
Oxygen
Thomson then discovered, using the same technology, that _______ charge particles existed in the atom.
Positively
What particles are in the nucleus of an atom?
Protons and Neutrons
The rays and particles emitted by radioactive material.
Radiation
Process (not requiring energy) by which unstable nuclei lose energy.
Radioactive Decay
Process whereby some substances spontaneously emit radiation.
Radioactivity
Who discovered the charge and mass of an electron with his oil drop experiment?
Robert Millikan
In this list, which substance can be classified as a chemical? a. salt b. sleep c. cold d. heat e. temperature
Salt
Who was instrumental in the discovery of the Cathode ray tube in the 1870's?
Sir William Crookes
The mass of an electron is what?
Smaller than the mass of a proton and neutron and a tiny fraction of the mass of an atom.
As the mass number of the isotopes of a particular element increases, the number of electrons ______.
Stays the same, as long as the charge is neutral. Changes, if the charge changes from neutral to positive or negative.
Dalton's theory soon had to be modified as _______ _____ were discovered.
Substance Particles
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.
The atomic mass will be between 35 and 37
Why did Rutherford expect Alpha particles to pass through the plum pudding model of the atom with little or no deflection?
The massive alpha particles were expected to be largely unaffected by the much less massive electrons. The diffusely, distributed positive charge inside the atom was also not expected to affect the positively charged alpha particles.
Describe the nucleus of an atom, as Rutherford concluded in his Gold Foil Experiment.
The nucleus is positively charged and dense.
An atom is electrically neutral because?
The number of protons and electrons are equal, and cancel each other out.
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.
The particles have fixed positions and are very close together.
The atomic mass of an atom is usually not a whole number because it accounts for what?
The relative abundance and the mass of each of the atom's isotopes.
The specific heat of copper is 0.092 cal/g °C, and the specific heat of silver is 0.057 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.
The silver will reach a higher temperature
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 linearly 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.
The temperature of steam cannot exceed 100 °C.
The mass number of an element is equal to what?
The total number of protons and neutrons in the atom's nucleus.
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.
They all have the same mass number.
How do isotopes hydrogen-1 and hydrogen-2 differ and relate?
They have 1 proton and H-2 has 1 proton, while H-1 has no protons.
What scientist described an atom made of solid positively charge substance with electrons dispersed throughout it?
Thomson
What scientist developed the plum pudding model?
Thomson
True or False: According to modern atomic theory, atoms of the same element may have different masses.
True
True or False:Atomic number is equal to the number of electrons in an atom.
True
True or False:Both Democritus and Dalton suggested that matter is made up of atoms.
True
True or False:Dalton thought that all atoms of specific elements have the same mass.
True
True or False:Dalton's atomic theory stated that atoms of different elements combine in simple whole-number ratios.
True
True or False:Dalton's atomic theory stated that atoms separate, combine, or rearrange in chemical reactions.
True
True or False:Neutrons have no electrical charge.
True
True or False:Philosophers formulated explanations about the nature of matter based on their own experiences.
True
True or False:The nucleus makes up most of atoms of the mass of the atom.
True
True or False:The number of protons in an atom identifies the atom as a particular element.
True
True or False:The periodic table is arranged by increasing atomic number.
True
What atomic model was thought to be true after Rutherford's Gold Foil Experiment? Which was thought to be false?
True-Wave Model (Electrons are distributed around the nucleus and occupy almost all the volume of the atom.) False-Plum Pudding Model (Electrons and protons even distributed throughout atom.)
True or False:Dalton's atomic theory was based on careful measurements and extensive research.
True.
Chlorofluorocarbons are broken down in the atmosphere by ________. a. nitrogen dioxide b. ozone c. iron d. AIDS e. ultraviolet light
UV Light
He used what to discover a negatively charged stream of _______?
Used a cathode ray tube to discover a negatively charge stream of matter.
The amount of space occupied by a substance is its... a. mass. b. density. c. weight. d. length. e. volume.
Volume
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.
a change in temperature of a solid
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.
all the protons and neutrons.
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.
are in the same group
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.
are unreactive and are rarely found in combination with other elements
The smallest particle of an element that retains the characteristics of the element is a(n) a. electron. b. neutron. c. proton. d. atom. e. nucleus.
atom
According to the atomic theory, a. all atoms are different. b. atoms are neither created nor destroyed during a chemical reaction. c. atoms of the same element combine to form compounds. d. all matter is made up of tiny particles called electrons. e. a compound can contain different numbers of atoms as long as it has the same kinds of atoms.
atoms are neither created nor destroyed during a chemical reaction
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
burning gasoline in a lawnmower
Which of the following is a chemical change? a. burning natural gas b. melting ice c. hammering gold into foil d. cutting a tomato e. cutting paper
burning natural gas
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
burning sugar
What elements are in hydroxyapatite, Ca5(PO4)3OH, 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
calcium, phosphorous, oxygen, hydrogen
Which of the following setups would convert centimeters to feet? a. cm x 2.54/1cm x 1ft/12in b. cm x 2.54cm/1in x 12in/1ft c. cm x 1in/2.54cm x 1ft/12in d. cm x 1in/2.54cm x 12in/1ft e. cm x 2.54cm/1in x 1ft/12in
cm x 1in/2.54cm x 1ft/12in
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
decreases going across a period
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
decreases going down within a group
Gold in a ring is a(n) a. compound. b. heterogeneous mixture. c. element. d. homogeneous mixture. e. none of the above
element
The phrase "ability to do work" is a definition of a. specific heat. b. energy. c. calorie. d. heating. e. cooling.
energy
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.
evaporation
The number of dots in the electron dot symbol of nitrogen is a. one. b. two. c. three. d. four. e. five.
five
The number of significant figures in the measurement of 45.030 mm is a. none. b. three. c. four. d. five. e. six.
five
The number of dots in the electron dot symbol of carbon is a. one. b. two. c. three. d. four. e. five.
four
Identify the metalloid in the following list. a. sulfur b. fluorine c. silver d. copper e. germanium
germanium
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. burning coal
grinding coffee beans
The energy associated with the motion of particles in a substance is called a. temperature. b. electrical energy. c. heat. d. chemical energy. e. potential energy.
heat
Identify the noble gas in the following list. a. helium b. nitrogen c. oxygen d. gold e. chlorine
helium
Coins in a piggy bank are an example of a(n) a. compound. b. heterogeneous mixture. c. element. d. homogeneous mixture. e. none of the above
heterogeneous
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.
in the outermost energy level of an atom
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
increases going down within a group
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
increases going down within a group
The number of valence electrons found in an atom of a Group A element is equal to a. its atomic number. b. its mass number. c. its group number. d. eight. e. eight minus the group number.
its group number
Which of the following is a measurement of mass in the metric system? a. milliliter b. centimeter c. kilogram d. Celsius e. meter
kilogram
Which of the following is the largest unit? a. millimeter b. micrometer c. meter d. decimeter e. kilometer
kilometer
The energy of motion is referred to as work. b. freezing. c. specific heat. d. potential energy. e. kinetic energy.
kinetic energy
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.
line dividing metals from nonmetals in the table
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
low melting points
Which of the following is the smallest unit? a. gram b. milligram c. kilogram d. decigram e. microgram
microgram
Which of the following elements is a nonmetal? a. nitrogen b. sodium c. iron d. silver e. calcium
nitrogen
Which of the following is a heterogeneous mixture? a. noodle soup b. water c. sugar d. tea e. carbon
noodle soup
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.
particles are close together and move randomly
The energy stored in chemical bonds is a. specific heat. b. kinetic energy. c. potential energy. d. work. e. a calorie.
potential energy
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
pouring water into a vacuum-insulated bottle
An example of kinetic energy is a coiled spring. b. running water. c. a tree. d. natural gas. e. chemical energy.
running water
What element has the electron arrangement 2,8,4? a. carbon b. oxygen c. sulfur d. iron e. silicon
silicon
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
steam at 110
The element in this list with chemical properties similar to magnesium is a. sodium. b. boron. c. carbon. d. strontium. e. chlorine.
stronium
Which of the following elements is a metal? a. nitrogen b. fluorine c. argon d. strontium e. phosphorus
strontium
Which of the following is a homogeneous mixture? a. noodle soup b. water c. sugar d. tea e. carbon
tea
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.
the changes in the temperature and physical state of a substance as it is heated.
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.
the coldest temperature possible.
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
the energy needed to remove the least tightly bound electron
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
the heat of vaporization for water
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.
the mass number - the atomic number
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 each energy level can hold.
the number of electrons in each energy level
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.
the number of protons plus neutrons
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.
the same atomic number but different numbers of neutrons.
A burn from steam at 100 °C is expected to be more severe than a burn 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.
the steam will give off a large amount of heat as it condenses.
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.
the valence electrons
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.
very large relative to the size of the molecules
A value of 36 mL is a measure of a. density b. mass c. temperature d. volume e. distance
volume
Raising the temperature of 10.0 g of water from 10.0 °C to 20.0 °C requires 100.0 cal of energy, while raising the temperature of 10.0 g of aluminum from 10.0 °C to 20.0 °C requires 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.
water has a larger specific heat than aluminum
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
water stored in a reservoir
The measurement of the gravitational pull on an object is its a. volume. b. weight. c. mass. d. length. e. size.
weight
