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WorksheetsChemical Bonds
Total questions: 35
Worksheet time: 18mins
Name
Class
Date
1.
In a chemical formula, the number of each type of atom in the compound is shown by numbers called _____?
a)
superscripts
b)
chemical symbols
c)
oxidation numbers
d)
subscripts
2.
A group of covalently bonded atoms that acts together as one charged atom is a ______.
a)
crystal
b)
molecule
c)
negative ion
d)
polyatomic ion
3.
The elements that make up a compound and the exact number of atoms of each element in a unit of the compound can be shown in a ____.
a)
chemical formula
b)
chemical symbol
c)
subscript
d)
superscript
4.
A chemical bond that occurs when atoms share electrons is a(n) ____ bond.
a)
covalent
b)
ionic
c)
magnetic
d)
polyatomic
5.
Name the following compound: CaBr2
a)
calcium bromide
b)
calcium bromine
c)
carbon bromine
d)
none of these
6.
The sum of the oxidation numbers in a neutral compound is always ____.
a)
a negative number
b)
one
c)
a positive number
d)
zero
7.
The oxidation number of an atom is shown with a ____.
a)
negative number
b)
positive number
c)
subscript
d)
superscript
8.
How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?
a)
2
b)
4
c)
6
d)
8
9.
What kind of chemical bond is formed when an exchange of electrons occurs?
a)
covalent
b)
hydrate
c)
ionic
d)
magnetic
10.
What is the total number of atoms in the compound Ca(ClO3)2?
a)
2
b)
3
c)
5
d)
9
11.
How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
a)
4
b)
7
c)
11
d)
12
12.
What is the name of the compound with the formula NaCl?
a)
chlorine sodiate
b)
sodium chlorate
c)
sodium chloride
d)
sodium dichloride
13.
Why do the noble gases NOT form compounds readily?
a)
They have empty outer energy levels.
b)
They have no electrons.
c)
They have seven electrons in the outer energy levels.
d)
Their outer energy levels are completely filled with electrons.
14.
What is the number of potassium atoms compared to oxygen atoms in a binary compound made from these two elements?
a)
One potassium atom to two oxygen atoms
b)
One potassium atom to three oxygen atoms
c)
Two potassium atoms to one oxygen atom
d)
Three potassium atoms to one oxygen atom
15.
What is the name of a binary compound made up of lithium and chlorine?
a)
chlorine lithiate
b)
chlorine lithium
c)
lithium chloride
d)
lithium chlorate
16.
Which of the following is the correct formula for magnesium nitrate?
a)
MgNO3
b)
Mg2NO3
c)
Mg(NO3)2
d)
Mg2(NO3)2
17.
What is the charge of phosphate in K3PO4?
a)
-7
b)
-3
c)
+1
d)
+4
18.
What is the correct name for K2SO4?
a)
potassium disulfide
b)
potassium sulfate
c)
potassium sulfide
d)
potassium(II) sulfate
19.
What is the correct formula for magnesium oxide?
a)
MgO
b)
MgO2
c)
Mg2O2
d)
Mg2O
20.
What type of bond is shown here?
a)
polar covalent
b)
ionic
c)
nonpolar covalent
d)
none of these
21.
A _____ is the force that holds atoms together in a compound.
a)
chemical bond
b)
strong nuclear force
c)
weak nuclear force
d)
none of these
22.
What happens to the electrons in a polar covalent bond. They are ____.
a)
equally shared
b)
unequally shared
c)
transferred
d)
none of these
23.
Most covalent compounds are _____ at room temperature.
a)
gases
b)
liquids
c)
solids
d)
gases or liquids
24.
Most ___ compounds are crystalline solids with high melting points.
a)
ionic
b)
non polar covalent
c)
polar covalent
d)
polar & non polar covalent
25.
The properties of a compound are __________ the properties of the elements making up the compound.
a)
different from
b)
the same as
26.
Because a water molecule has a slight positive charge at one end and a slight negative charge at the other end, it is a(n) _____ molecule.
a)
ionic
b)
non-polar
c)
polar
d)
none of these
27.
Molecules are usually _____.
a)
ionic
b)
electrically charged
c)
electrically neutral
d)
none of these
28.
A term that means "without water" is _____.
a)
ammoniated
b)
anhydrous
c)
hydrated
d)
none of these
29.
When an atom gains or loses electrons, the charged particle that results is called _____.
a)
a molecule
b)
an ion
c)
a polyatomic ion
d)
none of these
30.
The formula (SO4)-2 stands for _____.
a)
ammonium
b)
sulfate
c)
sulfide
d)
none of these
31.
The chlorine atoms in hydrogen chloride have a stronger attraction for the electrons than the hydrogen atoms do. The hydrogen chloride molecule is therefore a(n) _____ molecule.
a)
ionic
b)
non-polar
c)
polar
d)
none of these
32.
An element's _____ indicates how many electrons the element must gain, lose, or share to become stable.
a)
atomic number
b)
mass number
c)
oxidation number
d)
valence number
33.
The properties of a compound are the same as the properties of the elements making up the compound.
a)
True
b)
False
34.
Particles formed from the covalent bonding of atoms are called ions.
a)
True
b)
False
35.
When an atom gains or loses electrons, the charged particle that results is called a molecule.
a)
True
b)
False
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