Chemistry Review
Name:______________________________________________ Date:_________ Period:____
Place the correct answer on the line.
1. _____ In the equation 2 H2 + O2 → 2 H2O,
A) H2, O2, and H2O are all compounds.
B) H2, O2, and H2O are all elements.
C) only H2O is a compound.
D) only H2 and O2 are compounds.
E) H2, O2, and H2O are all trace elements.
2. _____ Which of the following particles is found in the nucleus of an atom?
A) protons and neutrons
B) protons and electrons
C) only neutrons
D) only protons
E) only electrons
3. _____ What is the atomic mass of an atom that has 6 protons, 6 neutrons, and 6 electrons?
A) 6
B) 8
C) +1
D) 12
E) 18
4. _____ An uncharged atom of boron has an atomic number of 5 and an atomic mass of 11.
How many electrons does boron have?
A) 11
B) 15
C) 0
D) 5
E) 2
5. _____ The sodium atom contains 11 electrons, 11 protons, and 12 neutrons. What is the mass
number of sodium?
A) 0
B) 11
C) 22
D) 23
E) 34
6. _____ A radioactive isotope is an isotope that
A) is stable.
B) decays.
C) has more protons than the common variant of the element.
D) has more electrons than the common variant of the element.
E) has the same atomic mass, but a different atomic number than the common variant of the
element.
7. _____ When full, the innermost electron shell of argon contains ________ electrons, and the
outermost shell contains ________ electrons.
A) 2 . . . 2
B) 2 . . . 8
C) 4 . . . 8
D) 8 . . . 2
E) 8 . . . 8
8. _____ What happens to an atom if the electrons in the outer shell are altered?
A) The atom becomes radioactive.
B) The atom will disintegrate.
C) The properties of the atom will change.
D) The atom will remain the same.
E) The atom's characteristics change and it becomes a different element.
9. _____ A(n) ________ forms when two atoms share electrons.
A) ion
B) element
C) covalent bond
D) ionic bond
E) hydrogen bond
10. _____ A hydrogen atom has one electron. How many covalent bonds can hydrogen form?
A) one covalent bond
B) four covalent bonds
C) four covalent bonds
D) two ionic bonds
E) two isotonic bonds
11. _____ What is the fundamental difference between covalent and ionic bonding?
A) In a covalent bond, the partners have identical electronegativity; in an ionic bond, one of
them is more electronegative.
B) In a covalent bond, the partners share a pair of electrons; in an ionic bond, one partner
accepts electrons from the other.
C) In covalent bonding, both partners end up with filled outer electron shells; in ionic
bonding, one partner does and the other does not.
D) Covalent bonding involves only the outermost electron shell; ionic bonding also involves
the next electron shell inside the outermost shell.
E) Covalent bonds form between atoms of the same element; ionic bonds form between
atoms of different elements.
12. _____ In the equation 2 H2 + O2 → 2 H2O, the H2 molecules are ________ and the H2O
molecules are ________.
A) reactants . . . products
B) products . . . reactants
C) created . . . destroyed
D) used . . . stored
E) destroyed . . . created
Use the diagram below to answer the next question.
13. _____ What change is occurring in this figure?
A) Sodium is gaining an electron.
B) Chlorine is losing an electron.
C) Sodium is becoming negatively charged.
D) Sodium is filling its third electron shell.
E) Chlorine is filling its third electron shell.
14. _____ About 25 of the 92 natural elements are known to be essential to life. Which four of
these 25 elements make up approximately 96% of living matter?
A) carbon, sodium, chlorine, nitrogen
B) carbon, sulfur, phosphorus, hydrogen
C) oxygen, hydrogen, calcium, sodium
D) carbon, hydrogen, nitrogen, oxygen
E) carbon, oxygen, sulfur, calcium
15. _____ Each element is unique and different from other elements because of the number of
protons in the nuclei of its atoms. Which of the following indicates the number of protons in
an atom's nucleus?
A) atomic mass
B) atomic weight
C) atomic number
D) mass weight
E) mass number
16. _____ Calcium has an atomic number of 20 and an atomic mass of 40. Therefore, a calcium
atom must have
A) 20 protons.
B) 40 electrons.
C) 40 neutrons.
D) A and B only
E) A, B, and C
17. _____ Which of the following best describes the relationship between the atoms described
below?
Atom 1
A)
B)
C)
D)
E)
Atom 2
They are isomers.
They are polymers.
They are isotopes.
They contain 1 and 3 protons, respectively.
They each contain 1 neutron.
18. _____ The atomic number of carbon is 6. Carbon-14 is heavier than carbon-12 because the
atomic nucleus of carbon-14 contains ____ neutrons.
A) 6
B) 7
C) 8
D) 12
E) 14
19. _____ Electrons exist only at fixed levels of potential energy. However, if an atom absorbs
sufficient energy, a possible result is that
A) an electron may move to an electron shell farther out from the nucleus.
B) an electron may move to an electron shell closer to the nucleus.
C) the atom may become a radioactive isotope.
D) the atom would become a positively charged ion, or cation.
E) the atom would become a negatively charged ion, or anion.
20. _____ From its atomic number of 15, it is possible to predict that the phosphorus atom has
A) 15 neutrons.
B) 15 protons.
C) 15 electrons.
D) 8 electrons in its outermost electron shell.
E) B and C only
Use the diagram below to answer questions 21 – 24.
21. _____ Which drawing depicts the electron configuration of oxygen (
A)
B)
C)
D)
E)
O)?
Drawing A
Drawing B
Drawing C
Drawing D
Drawing E
22. _____ Which drawing is of an atom with the atomic number of 6?
A) Drawing A
B) Drawing B
C) Drawing C
D) Drawing D
E) Drawing E
23. _____ Which drawing depicts an atom that is inert or chemically unreactive?
A) Drawing A
B) Drawing B
C) Drawing C
D) Drawing D
E) Drawing E
24. _____ Which drawing depicts an atom with a valence of 3?
A) Drawing A
B) Drawing B
C) Drawing C
D) Drawing D
E) Drawing E
Use the diagram below to answer questions 25 - 28.
25. _____ How many electrons does nitrogen have in its valence shell?
A) 2
B) 5
C) 7
D) 8
E) 14
26. _____ How many neutrons are present in the nucleus of a phosphorus atom?
A) 8
B) 15
C) 16
D) 31
E) 46
27. _____ Based on electron configuration, which of these elements would exhibit chemical
behavior most like that of oxygen?
A) carbon
B) hydrogen
C) nitrogen
D) sulfur
E) phosphorus
28. _____ Flourine has an atomic number of 9 and a mass number of 19. How many electrons
are needed to complete the valence shell of a fluorine atom?
A) 1
B) 3
C) 5
D) 7
E) 9
29. _____ If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen
(atomic number 1), which of the molecules below would be formed?
A) S-H
B) H-S-H
C) H-S-H
|
H
D)
H
|
H-S-H
|
H
E) H=S=H
30. _____ Which of the following describes any reaction that has attained chemical equilibrium?
A) The concentration of the reactants equals the concentration of the products.
B) The rate of the forward reaction is equal to the rate of the reverse reaction.
C) All of the reactants have been converted to the products of the reaction.
D) All of the products have been converted to the reactants of the reaction.
E) Both the forward and the reverse reactions have stopped with no net effect on
the concentration of the reactants and the products.