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WorksheetsChemistry, Chapter 7, Ionic & Metallic Bonding, Review
Total questions: 50
Worksheet time: 28mins
Name
Class
Date
1.
A mixture of two or more elements, at least one of which is a metal
a)
Alloy
b)
Halide ion
c)
Metallic Bond
d)
Ionic Compound
2.
The force of attraction binding oppositely charged ions together.
a)
Metallic Bond
b)
Covalent Bond
c)
Electromagnetic Attraction
d)
Ionic Bond
3.
The attraction of valence electrons for positive metal ions.
a)
Covalent Bond
b)
Metallic Bond
c)
Ionic Bond
d)
Electromagnetic Attraction
4.
A depiction of valence electrons around the symbol of an element.
a)
Electron Dot Diagram
b)
Bohr's Model
c)
Octet Rule
d)
Chemical Formula
5.
Compound of cations and anions.
a)
Ionic Compound
b)
Metallic Compound
c)
Ionic Bond
d)
Metallic Bond
6.
An anion of a halogen.
a)
Alloy
b)
Transition Metals
c)
Halide Ion
d)
Nonmetals
7.
An electron in the highest occupied energy level of an atom.
a)
Valence Electron
b)
Cation
c)
Anion
d)
Electron Dot Structure
8.
Atoms in most compounds tend to achieve the electron configuration of a noble gas.
a)
Ionization
b)
Ionic Bond
c)
Octet Rule
d)
Metallic Bond
9.
Shows the kinds and numbers of atoms in the smallest representative unit of a substance.
a)
Chemical Formula
b)
Formula Unit
c)
Chemical Compound
d)
Coordination Number
10.
Lowest whole-number ratio of ions in an ionic compound.
a)
Formula Unit
b)
Coordination Number
c)
Cation to Anion Ratio
d)
Octet Rule
11.
How many valence electrons does an atom of any element in Group 6A have?
a)
2
b)
4
c)
6
d)
8
12.
The electron dot structure for an atom of phosphorus is
a)
*
* P *
* P *
b)
* *
* P *
*
* P *
*
c)
* P *
d)
* *
: P *
* *
: P *
* *
13.
When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?
a)
2 +
b)
2 -
c)
3 +
d)
1 +
14.
The electron configuration of a fluoride ion, F-, is ____________________.
a)
1s22s22p5
b)
the same as that of the neon atom
c)
1s22s22p63s1
d)
the same as that of a potassium ion
15.
Metals are good conductors of electricity because they
a)
form crystal lattices
b)
contain positive ions
c)
contain mobile valence electrons
d)
form ionic bonds
16.
In forming chemical bonds, atoms tend to attain
a)
a state of higher energy
b)
the electron configuration of noble gas atoms
c)
the electron configuration of halogen atoms
d)
all of the above
17.
An ionic compound is
a)
electrically neutral
b)
held together by ionic bonds
c)
composed of anions and cations
d)
all of the above
18.
Which of these is NOT a characteristic of most ionic compounds?
a)
solid at room temperature
b)
has a low melting point
c)
conducts an electric current when melted
d)
produced by reaction between metallic and nonmetallic elements
19.
A metallic bond is a bond between
a)
valence electrons and positively charged metal ions
b)
the ions of two different metals
c)
a metal and nonmetal
d)
none of the above
20.
Which element when combined with chlorine would most likely form an ionic compound?
a)
Lithium
b)
Carbon
c)
Phosphorus
d)
Bromine
21.
A cation is any atom or group of atoms with
a)
a positive charge
b)
no charge
c)
a negative charge
d)
more electrons than the corresponding atom
22.
The cation Fe3+ is formed when
a)
an atom of iron loses two electrons
b)
an atom of zinc loses two electrons
c)
an atom of iron loses three electrons
d)
an atom of iron gains three electrons
23.
The chemical properties of an element are largely determined by the number of valence electrons the element has.
a)
Always true
b)
Sometimes true
c)
Never True
24.
Fluorine and chlorine each have one valance electron.
a)
Always true
b)
Sometimes true
c)
Never true
25.
Which is true about ionic compounds?
a)
They are good conductors because they are neutral.
b)
They are crystals because their electrons freely float.
c)
They have high melting points because cations and anions have strong attractions.
d)
They are malleable because they can be hammered without shattering.
26.
Which set of oxidation numbers are correct?
a)
Mg+2, O-3
b)
Sr+2, O-1
c)
Be+2, S-2
d)
Be-2, O+2
27.
Which statement is true?
a)
metals have a high boiling point because separating opposite charges takes a lot of energy.
b)
metals are malleable because the cations line up easily.
c)
metals are hard because they are solids.
d)
metals are conductors because they are not made of ions.
28.
A compound is found in the lab and has a crystal structure, a high melting point, and conducts electricity. How would it be classified?
a)
Ionic compound
b)
Covalent compound
c)
metallic compound
d)
a sea model
29.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
30.
Which is a characteristic of ionic compounds?
a)
They are solids at room temperature.
b)
They have a low melting point.
c)
They are not conductors.
d)
They involved electron sharing.
31.
Lithium Chloride with conduct electricity when...
a)
it is a solid.
b)
it is melted or dissolved in water.
c)
it is mixed with Hydrogen.
d)
it is a gas.
32.
Which of the following pairs of elements will form an ionic bond?
a)
K and Ca
b)
Co and Ni
c)
F and S
d)
Sr and Br
33.
Which IS a reason to use an alloy over a pure metal?
a)
Alloys are brittle compared to pure metals.
b)
Bronze is weaker than pure copper.
c)
Cast iron is heavy.
d)
Bronze is stronger and can withstand more heat than pure copper.
34.
When Magnesium forms a bond with Oxygen, what is the correct description?
a)
Magnesium loses 2 electrons forming a cation and Oxygen gains 2 forming an anion.
b)
Magnesium gains 2 electrons forming a cation and Oxygen loses 2 forming an anion.
c)
Magnesium loses 2 electrons forming a anion and Oxygen gains 2 forming an cation.
d)
Magnesium loses 3 electrons forming a cation and Oxygen gains 3 forming an anion.
35.
What is the oxidation number for a Sulfur atom?
a)
-1
b)
-2
c)
-3
d)
-4
36.
How many valence electrons does Nitrogen have?
a)
3
b)
4
c)
5
d)
6
37.
How many valence electrons does aluminum have?
a)
13
b)
14
c)
3
d)
4
38.
How many dots should be placed around silicone in a lewis dot structure?
a)
3
b)
4
c)
13
d)
14
39.
Magnesium's ion
a)
Mg+
b)
Mg2+
c)
Mg-
d)
Mg2-
40.
Rubidium (Rb) will likely _________ to reach a noble gas configuration.
a)
gain one electron
b)
gain two electrons
c)
lose two electrons
d)
lose one electron
41.
Why do ions form?
a)
Because electrons are repelled by the nucleus.
b)
Because the number of protons changes in the nucleus
c)
Because it is more stable for elements to have noble gas configurations.
d)
Because electrons degrade over time.
42.
An element forms an ion with a 2- charge. This means that 2 electrons were __________.
a)
Gained
b)
Lost
c)
Shared
d)
Destroyed
43.
An element always forms a cation with a 2+ charge. How many valence electrons did it have before it ionized?
a)
6
b)
1
c)
2
d)
5
44.
What is the electric charge of all ionic compounds?
a)
0
b)
+1
c)
+2
d)
+3
45.
When magnesium and chlorine react, they form an ionic compound. What is the charge of the ionic compound?
a)
+1
b)
+2
c)
-3
d)
0
46.
What salt forms when calcium and chlorine react?
a)
CaCl
b)
Ca2Cl
c)
CaCl2
d)
CaCl3
47.
CaO
a)
Calcium Oxygen
b)
Oxygen Calcium
c)
Oxygen Calcide
d)
Calcium Oxide
48.
Lithium Selenide
a)
LiSe
b)
Li2Se
c)
LiSe2
d)
Li2Se2
49.
The _________ never change in ions and neutral atoms.
a)
Neutrons
b)
Electrons
c)
Protons
d)
Atomic Mass
50.
What is the name of this polyatomic ion? OH-
a)
Hydroxide
b)
Cyanide
c)
Ammonium
d)
Peroxide
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