01 Problem Set

© 2013 Pearson Education, Inc.

1.1 Define isotopes.

a) Atoms with the same number of neutrons, but a different number of electrons

b) Atoms with the same number of protons, but a different number of electrons

c) Atoms with the same number of protons, but a different number of neutrons

d) Atoms with the same number of neutrons, but a different number of protons


a) Atoms with the same number of neutrons, but a different number of electrons

b) Atoms with the same number of protons, but a different number of electrons

c) Atoms with the same number of protons, but a different number of neutrons

d) Atoms with the same number of neutrons, but a different number of protons

1.1 Define isotopes.


1.2 Describe the structure of an atom.

a) Neutrons and protons are in the nucleus; electrons are in orbitals.

b) Neutrons and electrons are in the nucleus; protons are in orbitals.

c) Electrons and protons are in the nucleus; neutrons are in orbitals.

d) Electrons are in the nucleus; neutrons and protons are in orbitals.


a) Neutrons and protons are in the nucleus; electrons are in orbitals.

b) Neutrons and electrons are in the nucleus; protons are in orbitals.

c) Electrons and protons are in the nucleus; neutrons are in orbitals.

d) Electrons are in the nucleus; neutrons and protons are in orbitals.

1.2 Describe the structure of an atom.


1.3 What is the electronic configuration for Al?

a) 1s22s22p6

b) 1s22s22p63s1

c) 1s22s22p63s2

d) 1s22s22p63s23p1


a) 1s22s22p6

b) 1s22s22p63s1

c) 1s22s22p63s2

d) 1s22s22p63s23p1

1.3 What is the electronic configuration for Al?


1.4 What is the electronic configuration for Ca2+?

a) 1s22s22p63s2

b) 1s22s22p63s23p6

c) 1s22s22p63s23p64s2

d) 1s22s22p63s23p64s24p2


a) 1s22s22p63s2

b) 1s22s22p63s23p6

c) 1s22s22p63s23p64s2

d) 1s22s22p63s23p64s24p2

Explanation: Calcium has an electronic configuration of 1s22s22p63s23p64s2. The2+ means the loss of the last two electrons.

1.4 What is the electronic configuration for Ca2+?


1.5 Identify the compound with ionic bonding.

a) CH4

b) NaBr

c) CH3Cl

d) CH3OH


a) CH4

b) NaBr

c) CH3Cl

d) CH3OH

Explanation: Ionic bonds are formed between metals and nonmetals.

1.5 Identify the compound with ionic bonding.


1.6 How many bonding pairs of electrons are in NH2OH?

a) One pair of electrons

b) Two pairs of electrons

c) Three pairs of electrons

d) Four pairs of electrons






1.6 How many bonding pairs of electrons are in NH2OH?


1.7 How many nonbonding pairs of electrons are in NH2OH?










Explanation:NH2OH has one nonbonding pair on nitrogen and two nonbondingpairs on oxygen.

1.7 How many nonbonding pairs of electrons are in NH2OH?


1.8 How many bonds (pairs of electrons) are in CH2=CH2?

a) Two bondsb) Three bondsc) Four bonds

d) Five bondse) Six bonds


a) Two bonds

b) Three bonds

c) Four bonds

Explanation: CH2CH2 has two carbon–carbon bonds and four single carbon–hydrogen bonds.

1.8 How many bonds (pairs of electrons) are in CH2=CH2?

d) Five bonds

e) Six bonds


1.9 How does electronegativity change on the periodic table?

a) Increase from left to right; increase from top to bottom

b) Increase from left to right; increase from bottom to top

c) Increase from right to left; increase from top to bottom

d) Increase from right to left; increase from bottom to top


a) Increase from left to right; increase from top to bottom

b) Increase from left to right; increase from bottom to top

c) Increase from right to left; increase from top to bottom

d) Increase from right to left; increase from bottom to top

1.9 How does electronegativity change on the periodic table?


1.10 List the following atoms in order of decreasing electronegativity.

a) C > Br > O > F

b) F > O > C > Br

c) F > O > Br > C

d) F > C > O > Br


a) C > Br > O > F

b) F > O > C > Br

c) F > O > Br > C

d) F > C > O > Br

1.10 List the following atoms in order of decreasing electronegativity.


1.11 How many valence electrons does carbon have?

a) Three valence electrons

b) Four valence electrons

c) Five valence electrons

d) Six valence electrons

e) Seven valence electrons


a) Three valence electrons

b) Four valence electrons

c) Five valence electrons

d) Six valence electrons

e) Seven valence electrons

Explanation:Carbon has an electronic configuration of 1s22s22p2 and thus hasonly four electrons in its outer shell.

1.11 How many valence electrons does carbon have?


1.12 Identify the formal charge for C in CH3-.

a) -1

b) 0

c) 1

d) 2


a) -1

b) 0

c) 1

d) 2

1.12 Identify the formal charge for C in CH3-.


1.13 A compound has 85.72% carbon and 14.28% hydrogen. Give the empirical formula.

a) CH

b) CH2

c) CH3

d) CH4


a) CH

b) CH2

c) CH3

d) CH4

1.13 A compound has 85.72% carbon and 14.28% hydrogen. Give the empirical formula.


1.14 A compound has an EF of C2H5O and a MW of 90.121 g/mole. What is the MF?

a) C3H10O2

b) C4H8O

c) C4H10O2

d) C5H8O

e) C6H10O2


a) C3H10O2

b) C4H8O

c) C4H10O2

Explanation: Empirical weight of C2H5O is 45.06 g/mole. 90.121 / 45.06 = 2 C2x2H5x2O = C4H10O2

1.14 A compound has an EF of C2H5O and a MW of 90.121 g/mole. What is the MF?

d) C5H8O

e) C6H10O2


1.15 Identify the Arrhenius acid.HNO3 + H2O H3O+ + NO3

-

a) HNO3

b) H2O

c) H3O+

d) NO3-


a) HNO3

b) H2O

Explanation:

HNO3 dissociates in water to give H3O+ Arrhenius acid.

1.15 Identify the Arrhenius acid.HNO3 + H2O H3O+ + NO3

-

c) H3O+

d) NO3-


1.16 Identify the Brønsted–Lowry base.HCl + CH3NH2 CH3NH3

+ + Cl-

a) HCl

b) CH3NH2

c) CH3NH3+

d) Cl-


a) HCl

b) CH3NH2

Explanation:

CH3NH2 is a species that can accept a proton (Brønsted–Lowry base).

1.16 Identify the Brønsted–Lowry base.HCl + CH3NH2 CH3NH3

+ + Cl-

c) CH3NH3+

d) Cl-


1.17 Identify the Lewis base.

CH3O- + CH3Br CH3OCH3 + Br-

a) CH3O-

b) CH3Br

c) CH3OCH3

d) Br-


a) CH3O-

b) CH3Br

Explanation:

CH3O- is a species with nonbonding electrons that can be donated

to form new bonds (Lewis base).

1.17 Identify the Lewis base.

CH3O- + CH3Br CH3OCH3 + Br-

c) CH3OCH3

d) Br-


1.18 Identify the strongest acid.

a) H2O

b) CH3OH

c) CH3COOH

d) HF


a) H2O

b) CH3OH

Explanation: The acids decrease in strength in the order of

HF > CH3COOH > CH3OH > H2O.

1.18 Identify the strongest acid.

c) CH3COOH

d) HF


1.19 Identify the strongest base.

a) NH3

b) HCOO-

c) CH3-

d) OH-


a) NH3

b) HCOO-

Explanation: The bases decrease in strength in the order of CH3

- > OH- > NH3 > HCOO-.

1.19 Identify the strongest base.

c) CH3-

d) OH-


1.20 Define a nucleophile.

a) A species that donates electrons

b) A species that accepts electrons

c) A species that accepts protons

d) A species that donates protons


a) A species that donates electrons

b) A species that accepts electrons

c) A species that accepts protons

d) A species that donates protons

Explanation:

A nucleophile donates electrons, and an electrophile accepts electrons.

1.20 Define a nucleophile.

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