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BM2 review

Total questions: 87

Worksheet time: 2hrs 56mins

Name
Class
Date
1.
Ammonium
a)
NH4+
b)
NO3-
c)
NO2-
d)
MnO4-
2.
Carbonate
a)
Cr2O4-2
b)
CH3COO-
c)
CO3-2
d)
CN-
3.
Cyanide
a)
CrO4-2
b)
Cr2O4-2
c)
CO3-2
d)
CN-
4.
Hydroxide
a)
Cr2O4-2
b)
Cr2O4-2
c)
O3-2
d)
OH-
5.
Phosphate
a)
PO4-3
b)
O2-2
c)
OH-
d)
CO3-2
6.
acetate
a)
C2H3O21-
b)
C3H2O31-
c)
C2H2O31-
d)
C3H3O21-
7.

Mg(NO3)2

a)

magnesium nitrate

b)

magnesium nitrite

c)

magnesium nitride

d)

magnesium nitrogen oxide

8.

Ga(CN)3

a)

gallium cyanide

b)

gallium carbon nitride

c)

gallium (III) cyanide

d)

gallium carbon trinitride

9.

Ca(PO4)3

a)

calcium phosphate

b)

calcium phosphite

c)

calcium phosphide

d)

calcium (II) phosphorus oxide

10.

ammonium sulfide

a)

(NH4)2S

b)

NH4S

c)

(NH4)2SO4

d)

NH4(S)2

11.

sodium nitrate

a)

NaNO3

b)

Na(NO3)

c)

NaNO2

d)

Na(NO)2

12.
The name of the compound NH4F is
a)
Nitrogen hydrogen fluorine
b)
Ammonium Fluoride
c)
Ammonia Fluoride
d)
Nitrogen tetrahydride fluoride
13.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
14.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
15.
The name of Fe(OH)₂ is
a)
iron oxide
b)
iron hydroxide
c)
iron (II) hydroxide
d)
iron dihydroxide
16.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
17.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
18.

When naming ionic compounds, write the cation as it is written on the periodic table and write the anion with which ending?

a)

-ite

b)

-ate

c)

-ide

d)

-ade

19.

What is the charge (oxidation number) for sulfur?

a)

+2

b)

-2

c)

-6

d)

+3

20.

What is the formula for zinc fluoride?

a)

ZnF

b)

ZnF2

c)

Zn2F

d)

ZnF4

21.

Write the name for PbO2

a)

lead oxide

b)

lead (II) oxide

c)

lead (IV) oxide

d)

lead (II) peroxide

22.

Write the formula for Fe(C2H3O2)3

a)

iron acetate

b)

iron (III) acetate

c)

iron oxalate

d)

iron (III) oxalate

23.

Write the name for Ag2CO3

a)

silver carbonate

b)

silver (I) carbonate

c)

gold carbonate

d)

silver oxalate

24.
What line segment represents only the solid state?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
25.
Which segment represents the heat of fusion?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
26.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
27.
Which process takes the longest to occur?
a)
melting
b)
boiling
c)
freezing
d)
heating the solid
28.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
29.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
30.
Between which points is the temperature of the substance increasing?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
31.
Between which points is the substance changing state?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
32.
This type of graph is called a:
a)
Phase diagram
b)
Heating curve
c)
State of matter
d)
Temperature chart
33.

Which two particles are attracted to each other?

a)

Two neutrons

b)

A proton and an electron

c)

Two protons

d)

An electron and a neutron

34.

A repulsive force exists between which two particles?

a)

Two neutrons

b)

An electron and a neutron

c)

An electron and a proton

d)

Two protons

35.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
36.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have less mass

c)

the atoms have a bigger effective nuclear charge

d)

the atoms have less electrons.

37.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

38.

Which of these has the largest atomic radius?

a)

oxygen

b)

fluorine

c)

sulfur

d)

chlorine

39.

Which of these elements has the smallest atomic radius?

a)

C

b)

Ne

c)

K

d)

Al

e)

P

40.

Atomic radius generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

41.

The effective nuclear charge of magnesium is

a)

+1

b)

+2

c)

+12

d)

+24

42.

Effective nuclear charge ________ across a period.

a)

increases

b)

decreases

c)

stays the same

43.

Why does Ca have a larger radius than Se?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

44.

Which of the following elements has the most "shielding" electrons?

a)

nitrogen

b)

phosphorus

c)

arsenic

d)

bismuth

45.

In the following configuration, which electrons are the core electrons? 1s2 2s2 2p6 3s2 3p4

a)

1s2 2s2 2p6

b)

3s2 3p4

c)

1s2 2s2

d)

2s2 2p6 3s2 3p4

46.
The valence electrons are located on 
a)
the orbital closest to the nucleus
b)
the orbital furthest from the nucleus
c)
the orbital with the most electrons
d)
the orbital with the least electrons
47.
What creates a SHIELDING EFFECT by interfering with the attractive forces between the protons and the electrons.
a)
nucleus
b)
valence electrons
c)
core electrons
d)
protons
48.
As you move across a period (row), the shielding effect
a)
increases by a factor of 2
b)
decreases by a factor of 2
c)
stays constant
d)
alternates for metals an nonmetals
49.
What is the Nuclear charge of yttrium? 
a)
40
b)
41
c)
38
d)
39
50.
What is EFFECTIVE nuclear charge
a)
The charge that actually matters
b)
The sharge of an element
c)
The charge felt by the valence electrons
d)
The charge felt by the inner orbital electrons
51.
In the following configuration, which electrons are the shielding electrons? 1s2 2s2 2p6 3s2 3p4
a)
1s2 2s2 2p6
b)
3s2 3p4
c)
1s2 2s2
d)
2s2 2p6 3s2 3p4
52.

What is the effective nuclear charge on alkaline earth metal atoms?

a)

+2

b)

+1

c)

+3

d)

+6

53.

How many "dots" are used in a dot diagram of a nitrogen atom?

a)

5

b)

7

c)

2

d)

8

54.

What are the vertical columns on the periodic table called

a)

Groups

b)

Periods

c)

Exclamation Points

d)

Cliques

55.

What are the horizontal rows on the periodic table called

a)

Groups

b)

Periods

c)

Exclamation Points

d)

Cliques

56.

Which property is the size of an atom

a)

Atomic Radius

b)

Effective Nuclear Charge

c)

Ionization Energy

d)

Electronegativity

57.

Which property is the energy to remove an electron

a)

Electron Affinity

b)

Effective Nuclear Charge

c)

Ionization Energy

d)

Electronegativity

58.

Which property is the attraction for other atom's valence electrons?

a)

Electron Affinity

b)

Effective Nuclear Charge

c)

Ionization Energy

d)

Electronegativity

59.

Because Noble Gases do not want to change their number of electrons, they have the _________________ a period.

a)

lowest ionization energies but the highest electron affinities

b)

highest ionization energies but the lowest electron affinities

c)

lowest ionization energies and electron affinities

d)

highest ionization energies and electron affinities

60.

Which of the following would have a greater effective nuclear charge?

a)

An atom with 10 protons.

b)

An atom with 20 protons.

c)

An atom with 15 electrons.

d)

An atom with 5 electrons.

61.

Which of the following is responsible for the effective nuclear charge?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Photons

62.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
63.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
64.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
65.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
66.

This orbital diagram represents:

a)

Carbon

b)

Boron

c)

Nitrogen

d)

Oxygen

67.

Which example shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

68.

Which of the following is written correctly?

a)

A

b)

B

c)

C

d)

D

69.

An aluminum ion would have which electron configuration?

a)

[1s2 2s2 2p6 3s2]+3

b)

[1s2 2s2 2p6 3s2 3p1]+3

c)

[1s2 2s2 2p6 3s2 3p6]_3

d)

[1s2 2s2 2p6]+3

70.

Which ion has this electron configuration [1s22s22p63s23p6]

a)

Na+

b)

O2-

c)

P3-

d)

Rb+

71.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
72.

Which of the following elements is located in the "p" block of the periodic table?

a)

Sc

b)

Ca

c)

Se

d)

Sm

73.

Which of the following elements has the largest atomic radius?

a)

Cl

b)

S

c)

Br

d)

As

74.

Pick the atom from each pair listed below that has the larger atomic radius:

a. Be or Ba b. Si or S c. Ga or B d. Sr or Ag

a)

Ba, Si, Ga, and Sr

b)

Be, S, B, and Ag

c)

Be, Si, Ga, and Ag

d)

Ba, S, B, and Sr

75.

Compare the following ions with their neutral atom and choose the ones with the larger radius of each set.

Ba2+ or BaBa^2+\ or\ Ba Br− or BrBr^-\ or\ Br Al+3 or AlAl^{+3\ }or\ Al O−2  or OO^{-2}\ \ or\ O

a)

Ba, Br−1, Al, and O−2Ba,\ Br^{-1},\ Al,\ and\ O^{-2} Ba, Br-1, Al, and O-2

b)

Ba, Br, Al, and O

c)

Ba, Br, Al, and O

76.

What is the trend for ionic radius across a period for anions?

a)

increase

b)

decrease

c)

remain constant since they are all the same type of ion

77.

What is the trend for ionic radius across a period for cations?

a)

increase

b)

decrease

c)

remain constant since they are all the same type of ion

78.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

79.

Which is the smaller atom: Mg or Mg+2?

a)

Mg because it gains an energy level since it gains 2 electrons.

b)

Mg due to extra electron repulsion created by gaining 2 electrons.

c)

Mg+2 because of extra electron repulsion created by gaining 2 electrons.

d)

Mg+2 because it loses an energy level since it loses 2 electrons.

80.

Arrange the following by decreasing ionic radius: Ag+1, In+3, Cd+2, Sn+4?

a)

Ag+1, In+3, Cd+2, Sn+4

b)

Ag+1, Cd+2, In+3, Sn+4

c)

Sn+4, In+3, Cd+2, Ag+1

d)

Sn+4, Cd+2, In+3, Ag+1

81.

Which is the larger atom? Ca+2, K+1, Ga+3?

a)

Ca+2

b)

K+1

c)

Ga+3

d)

they are all the same size since they are all cations

82.

Which is the larger atom: F-1, Cl-1, Br-1?

a)

F-1

b)

Cl-1

c)

Br-1

d)

they are all the same size since they are all anions

83.

This circles in this diagram could represent

a)

Sulfur

b)

Potassium

c)

Phosphorous

d)

Bromine

84.

What is the example of species that are isolectronic?

a)

Na+ and Si4+

b)

Na+ and Cl-

c)

Mg2+ and Al +

d)

S2- and O2-

85.

What is meant by isolectronic?

a)

Group of atoms or ions that have the same electronic configuration

b)

Group of atoms or ions that have the same protonic configuration

c)

Group of atoms or ions that have the same electrical properties

d)

Group of atoms or ions that have the same electron charge

86.

Arrange these species in increasing order of size.

Cl- , Ca2+ , S2- , Ar , K+

a)

Ca2+ > K+ > Ar > Cl- > S2-

b)

S2- > Cl- > Ar > K+ > Ca2+

c)

Ca2+ < K+ < Ar < Cl- < S2-

d)

S2- < Cl- < Ar < K+ < Ca2+

87.

Na+ and Al3+ are isoelectronic species (1s2 2s2 2p6). Which of these ion is smaller?

a)

Na+

b)

Al3+

c)

I'm not sure

d)

They have the same size

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