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Q3 Mini #2: Trends, Bonding and Naming Compounds

Total questions: 78

Worksheet time: 1hrs 4mins

Name
Class
Date
1.
What is the name of Group 1?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
2.
What is the name of Groups 18?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Halogens
d)
Noble Gases
3.

How does the atomic radius change across a period ?

a)

increases

b)

decreases

c)

stays the same

4.

How does the ionization energy change across a period ?

a)

increases

b)

decreases

c)

stays the same

5.

how does the electronegativity change across a period ?

a)

increases

b)

decreases

c)

stays the same

6.

how does the electronegativity change down a group ?

a)

increases

b)

decreases

c)

stays the same

7.

which of the following has the smallest atomic radius ?

a)

Li

b)

K

c)

Na

d)

Cs

8.

Which atom has the least electronegativity ?

a)

Cs

b)

Li

c)

Na

d)

K

9.

Which of these elements would require the MOST energy to remove its outermost electron?

a)

Krypton (Kr)

b)

Potassium (K)

c)

Iron (Fe)

d)

Germanium (Ge)

10.

Which of the following will have a LESS ionization energy than magnesium (Mg, atomic #12)?

a)

Helium (He)

b)

Beryllium (Be)

c)

Radium (Ra)

d)

Sodium (Na)

11.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
12.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

13.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
14.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
15.
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 more protons.
d)
the atoms have less electrons.
16.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
17.

Rank these elements from smallest atomic radius to largest atomic radius: Ag, Au, Cu, Rg

a)

Ag, Au, Cu, Rg

b)

Au, Ag, Rg, Cu

c)

Rg, Au, Ag, Cu

d)

Cu, Ag, Au, Rg

18.

Which element would have the same number of energy levels as Zinc (Zn, atomic #30)?

a)

Cadmium

b)

Krypton

c)

Silver

d)

Tin

19.

The horizontal rows on the periodic table, which indicate the number of energy levels/orbitals that an atom has, are called ___________.

a)

Periods

b)

Element

c)

Atomic Number

d)

Group

20.

The atomic radius of an atom describes its _________________.

a)

size

b)

reactivity

c)

color

d)

luster

21.

_____________________________ describes the energy needed to remove the outermost electron from an atom and make it an ion.

a)

atomic radius

b)

ionization energy

c)

electronegativity

d)

malleability

22.

Electronegativity describes the tendency of an atom to _______________ electrons toward it when it is bonded to another atom.

a)

release

b)

pull

c)

absorb

23.

What would be an accurate title for this periodic table?

a)

Trend in Metallic Properties

b)

Trend in Ionization Energy

c)

Trend in Electronegativity

d)

Trend in Atomic Radius

24.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
25.
What is the charge on an Aluminium ion?
a)
3
b)
+3
c)
+2
d)
+1
26.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
27.
What is the charge of Neon?
a)
0
b)
+1
c)
-1
d)
1
28.
How many valence electrons does hydrogen have?
a)
1
b)
2
c)
3
d)
4
29.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
30.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
31.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
32.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
33.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
34.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
35.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
36.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
37.
What will be the compound name of the following chemical formula?
NaCl
a)
Potassium Chloride
b)
Sodium Chloride
c)
Calcium Chloride
d)
Sodium Chlorine
38.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
39.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
40.
which types of elements become cations?
a)
nonmetals
b)
all metals
c)
only transition metals
d)
some metals and some metalloids
41.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
42.
What is the formula of calcium oxide?
a)
CaO2
b)
CaO
c)
Ca2O
d)
CO
43.
How many electrons has an oxide ion lost?
a)
1
b)
2
c)
6
d)
0
44.
What are ionic bonds?
a)
valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
45.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
46.
When the number of electrons equals the number of protons the atom has what charge?
a)
sponge bob
b)
positive charge
c)
negative charge
d)
neutral charge
47.
What is released when an ionic bond forms?
a)
butterflies
b)
cats
c)
dogs
d)
energy
48.
How do positive ions form?
a)
by gaining electrons
b)
getting compliments
c)
by losing electrons
d)
gaining more protons
49.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
50.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
51.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
52.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
53.

Which of the following is a covalent bonding?

a)

MgS

b)

NaCl

c)

CH4

d)

LiBr

54.

What characteristic differentiates covalent bonding from ionic bonding?

a)

Electrons are transferred from one atom to another to form a bond

b)

Electrons are shared in pairs from one atom to another to form a bond

55.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
56.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
57.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
58.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
59.
How many valence electrons do most atoms need to be stable?
a)
1
b)
2
c)
6
d)
8
60.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
61.
In the correct Lewis Structure for methane (CH4), how many unpaired electrons can be found around Carbon?
a)
0
b)
2
c)
4
d)
8
62.

How many electrons are shared in a single covalent bond?

a)

2 pairs

b)

4

c)

2

d)

1

63.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
64.

Which is stronger...

a)

N − N

b)

N = N

c)

N ≡ N

65.

A double bond between 2 carbon atoms is the same strength as 2 single bonds between carbon atoms.

a)

true

b)

false

66.
Determine the type of bond in an oxygen molecule (O2). HINT: Use (IE - AE)/2 = # of bonds.
a)
Double covalent
b)
Single covalent
c)
Ionic
d)
Triple covalent
67.
Determine the type of bond in a nitrogen molecule (N2). HINT: Use (IE - AE)/2 = # of bonds.
a)
Double covalent
b)
Single covalent
c)
Ionic
d)
Triple covalent
68.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
69.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
70.
CO2
a)
Ionic 
b)
Covalent
71.
cation + anion
a)
Ionic 
b)
Covalent
72.

Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

73.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
74.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
75.
What is the chemical formula for dinitrogen tetraoxide?
a)
N4O2
b)
NO4
c)
N2O4
d)
N2O
76.
What is the name of S2Br6?
a)
sulfur hexabromide
b)
disulfur hexabromine
c)
disuflur hexabromide
d)
disulfur pentabromide
77.
What is the chemical formula for carbon monoxide?
a)
CO2
b)
CO
c)
CO3
d)
C2O
78.
SO
a)
sulfur oxide
b)
sulfur monoxide
c)
monosulfur monoxide
d)
monosulfur oxide

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