Chapter 1
1. What is the difference between an atom and an element?
A. An atom is the smallest unit of an element, and an element is a pure substance that
cannot be broken down.
B. An atom is a pure substance that cannot be broken down, and an element is the
smallest unit of an atom.
C. An atom and an element are the same thing.
D. None of the above
2. What is a pure substance? Give an example.
A. A pure substance has a fixed composition. Hydrogen
B. A pure substance has a fixed composition. Hydrogen and Hydrogen
C. A pure substance is a blend of two or more kinds of matter. Hydrogen and Carbon
D. A and B
3. What is the difference between extensive and intensive properties?
A. An extensive property depends on amount, and an intensive property doesn’t depend
on amount.
B. An extensive property doesn’t depend on amount, and an intensive property does
depend on amount.
C. They both depend on the amount.
D. None of the above
4. Which of the following is not an element?
A. Phosphorus
B. Hafnium
C. Aluminum
D. Frandium
5. What is the difference between a liquid and a gas?
A. A liquid has a definite shape, and a gas has a definite volume.
B. A liquid has definite volume, and a gas has no definite volume or shape.
C. A liquid has a definite shape and volume, a gas has neither.
D. A gas has a definite shape and volume, a liquid has neither.
6. Which of the following is an example of a mixture?
A. Water
B. Sodium Chloride
C. Sugar in water
D. Sucrose
7. Which of these is a physical property?
A. pH
B. Reactivity with water
C. Melting point
D. Producing a gas
Chapter 2
1. What is the difference between accuracy and precision?
A. Accuracy is closest to the point, and precision is close together.
B. Precision is the closest to the point, and accuracy is the closest together
C. Accuracy is the same thing as precision
D. None of the above
2. How many sig figs are in 67.029?
A. 4
B. 3
C. 5
D. 2
3. A student measures the mass and volume of a substance, and calculates its density as 6.23
gallons/mL. The accepted value of the density is 7.1 gallons/mL. What is the percentage error of
the student's measurement? Round your answer to the nearest tenth.
A. 5 %
B. 13%
C. 9%
D. 12.3 %
4. Calculate the density if the mass is 12.6 g, and the volume is 7.38 mL3. Round your answer to
the nearest tenth.
A. 1.7 g/mL3
B. 2.3 g/mL3
C. 2.2 g/mL3
D. 3.4 g/mL3
5. What is the difference between directly and inversely proportional?
A. Directly proportional is when you divide one by the other and get a constant value.
Inversely proportional is when the product of the quantities is constant.
B. Inversely proportional is when you divide one by the other and get a constant value.
Directly proportional is when the product of the quantities is constant.
C. They are the same thing.
D. None of the above
6. What is the first step of the scientific method?
A. Hypothesis
B. Draw Conclusions
C. Observe
D. Test
7. If you have 38 milligrams of chocolate, how many grams of chocolate do you have?
A. 0.038 grams
B. 0.38 grams
C. 3.8 grams
D. 0.0038 grams
Chapter 3
1. Which of the following isn’t a fundamental law of chemistry?
A. The Law of Conservation of Mass
B. The Law of Definite Proportions
C. The Law of Multiple Proportions
D. The Law of Gravity
2. Which one of Dalton’s theories is no longer valid?
A. In chemical reactions atoms are combined, separated, or rearranged.
B. Atoms of different elements combine in simple whole number ratios to form chemical
compounds.
C. Atoms of a given element are identical to each other.
D. All matter is composed of atoms.
3. What scientist came up with the atomic theory?
A. Rutherford
B. Dalton
C. J.J. Thomson
D. Mrs. Mullane
4. Who came up with the nuclear model?
A. Rutherford
B. Bohr
C. Dalton
D. J.J. Thomson
5. Who created the planetary model?
A. Bohr
B. Rutherford
C. Dalton
D. J.J. Thomson
6. What subatomic particle has a negative charge?
A. Proton
B. Electron
C. Neutron
D. Isotope
7. If you have 4 protons and 6 neutrons, what is the atomic mass of the atom?
A. 3
B. 11
C. 2
D. 10
Chapter 4
1. What is the photoelectric effect experiment?
A. It was an experiment to figure out if light was a wave
B. It was an experiment to figure out if light was a particle
C. A and B
D. None of the above
2. Of the following, who didn’t contribute to the quantum model?
A. De Broglie
B. Heisenberg
C. Bohr
D. Schrödinger
3. What is the shape of a “p” orbital?
A. Circle
B. 4 leaf Clover
C. Figure 8
D. complex
4. Which of the following violates the four rules of filling orbitals with electrons?
A. Two electrons spinning in opposite directions
B. Two electrons spinning in the same direction
C. Filling the “s” orbital of the next energy level before filling the “d” orbital of the
current energy level
D. Hund’s Rule
5. What is the difference between valence and inner core electrons?
A. Valence electrons are in the inside energy levels, and inner core electrons are in the
outer energy level.
B. Valence electrons are in the outer energy level, and inner core electrons are in the
inside energy levels.
C. They are the same thing.
D. None of the above
6. What color has the longest wavelength?
A. Red
B. Blue
C. Violet
D. Green
7. Who performed the Hydrogen Line Emission?
A. Einstein
B. De Broglie
C. Schroedinger
D. Bohr
Chapter 5
1. What is the definition of periodic law?
A. Trends that don’t repeat
B. How electronegativity moves across the periodic table
C. The size of an atom measured by the distance between two neighboring atoms
D. Trends that repeat
2. What was Mendeleev’s nickname?
A. Mende
B. The Laughing Philosopher
C. The Father of the Modern Periodic Table
D. The Father of Modern Chemistry
3. What did Moseley do for modern chemistry?
A. He organized the periodic table by atomic mass
B. He organized the periodic table by atomic number
C. He organized the elements by property
D. None of the above
4. How does Ionization energy travel along the periodic table?
A. It increases across a period and decreases down a group.
B. It decreases across a period and increases down a group.
C. It decreases across a period and down a group.
D. It increases across a period and down a group.
5. What’s the difference between an atom and an ion?
A. An ion is the smallest unit of matter, and an atom is an element that has a charge.
B. An atom and an ion are the same thing.
C. An atom is the smallest unit of matter, and an ion is an atom that has a charge.
D. None of the above
6. Which of the following isn’t something to remember when explaining trends?
A. The power of the nucleus
B. The distance of valence electrons from the nucleus
C. The number of inner core electrons
D. The size of the atom
7. What is electron affinity?
A. In a compound, an atom’s ability to draw electrons closer to it.
B. It’s an atom’s ability to attract electrons.
C. The energy needed to remove an electron.
D. The size of an atom measured by the distance between two neighboring atoms.
Chapter 6
1. What’s one difference between ionic and covalent bonding?
A. There is no difference
B. Ionic is the transfer of electrons, and covalent is the sharing of electrons
C. Ionic is the sharing of electrons, and covalent is the transfer of electrons
D. Ionic has a low E.N.D., and covalent has a high E.N.D.
2. Which isn’t a type of bonding?
A. Ionic
B. Covalent
C. Metallic
D. Emotional
3. What is an IMF?
A. Igloos Melting Fast
B. Intermolecular Forces
C. Injured Molecular Forces
D. Iguanas Make Friends
4. What is a type of IMF?
A. London Dispersion Forces
B. Dipole- Dipole
C. Hydrogen Bond
D. All of the above
5. What is the purpose of a chemical bond?
A. To get to a lower potential energy
B. To get to a better stability
C. A and B
D. None of the above
6. What is one way to determine the strength of an ionic bond?
A. The charge of the ions involved
B. The bond type
C. The bond length
D. None of the above
7. Which element is never a central atom in a Lewis Structure?
A. C and D
B. Carbon
C. Fluorine
D. Hydrogen
Chapter 7
1. What types of elements are in covalent compounds?
A. Two nonmetals
B. A nonmetal and a metal
C. Two metals
D. A metal and a polyatomic ion
2. Which type of compound uses Greek prefixes?
A. Ionic- a metal and a nonmetal
B. Ionic- a metal and a PAI
C. Covalent
D. None of the above
3. What is the name for the formula N2O5?
A. Nitrogen Monoxide
B. Nitrogen Oxide
C. Trinitrogen heptaoxide
D. Dinitrogen pentaoxide
4. What is the formula for Strontium Nitrate?
A. Sr2NO3
B. Sr(NO3)2
C. NO3Sr
D. SrNO3
5. What is the third step to finding the formula of a compound from the percent composition?
A. Mass to mole
B. Multiply till whole
C. Percent to mass
D. Divide by smallest
Answer Key
Chapter 1
1. A 4. D 7. C
2. D 5. B
3. A 6. C
Chapter 2
1. A 4. A 7. A
2. C 5. A
3. D 6. C
Chapter 3
1. D 4. A 7. D
2. C 5. A
3. B 6. B
Chapter 4
1. A 4. B 7. D
2. C 5. B
3. C 6. A
Chapter 5
1. D 4. A 7. B
2. C 5. C
3. B 6. D
Chapter 6
1. B 4. D 7. A
2. D 5. C
3. B 6. A
Chapter 7
1. A 4. B
2. C 5. D
3. D