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WorksheetsIonic Bonding Test
Total questions: 65
Worksheet time: 3615secs
Name
Class
Date
1.
Refer to the image. Which diagrams correctly represent the transfer of electrons in ionic bonding?
a)
Diagram 3 and 4
b)
Diagram 1 and 2
c)
Diagram 1 and 4
d)
Diagram 2 and 3
2.
What is the correct name of CaBr2?
a)
calcium bromine
b)
calcium baride
c)
monocalcium dibromide
d)
calcium bromide
3.
In the compound aluminum oxide, which is the cation?
a)
Al+3
b)
Al
c)
O-2
d)
O
4.
For the ions shown in the cartoon, the strongest force of attraction would be formed between.
a)
Li + and F -
b)
Na + and Cl -
c)
Cs + and F -
d)
Cs + and Br -
5.
Which of the following is NOT a property of ionic compounds?
a)
They conduct electricity when molten
b)
They conduct electricity when in solution
c)
They have high boiling points
d)
They are insoluble in water
6.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
7.
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
8.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
9.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
10.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
11.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
12.
Definition: the electrostatic attraction between positive and negative ions in a compound
a)
chemical bond
b)
atomic bond
c)
covalent bond
d)
ionic bond
13.
Alkali metal elements will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
14.
Definition: the simplest whole number ratio of atoms or ions of the elements in anionic compound
a)
formula unit
b)
atomic unit
c)
chemical unit
d)
ionic unit
15.
Pure ionic compounds are _____
a)
electrically neutral
b)
charged positively
c)
charged negatively
d)
strongly charged
16.
The most common model of ions shows them as spheres arranged in a regular three-dimensional pattern called _____
a)
a crystal lattice
b)
a wireframe lattice
c)
a crystal cube
d)
an ordered pair
17.
Concerning their physical properties, ionic substances are often _____
a)
hard and brittle
b)
soft and brittle
c)
hard and malleable
d)
soft and malleable
18.
A group 16 element will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
19.
Predict the charge on the most stable ion formed by calcium
a)
1+
b)
1-
c)
2+
d)
2-
20.
Predict the charge on the most stable ion formed by phosphorus
a)
1+
b)
1-
c)
2+
d)
3-
21.
Name this compound:
NiPO4
NiPO4
a)
Nickel (I) phosphate
b)
Nickel (II) phosphate
c)
Nickel (IV) phosphate
d)
Nickel (III) phosphate
22.
calcium hydroxide
a)
Ca2OH
b)
CaOH2
c)
Ca(OH)2
d)
correct answer is not given
23.
The correct formula for MnO4 - and Ca+2
a)
(MnO4)2Ca
b)
MnO4Ca2
c)
Ca2MnO4
d)
Ca(MnO4)2
24.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
25.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
lead + oxygen
26.
lithium permanganate
a)
LiMnO4
b)
MnO4Li
c)
Li4MnO
d)
correct answer is not given
27.
calcium phosphate
a)
Ca3P2O8
b)
Ca2(PO4)3
c)
CaPO4
d)
correct answer is not given
28.
Cu2CO3
a)
copper carbonate
b)
copper (II) carbonate
c)
copper (I) carbonate
d)
copper carbon oxide
29.
iron (II) sulfate
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
30.
copper (II) hydroxide
a)
CuOH2
b)
Cu2OH
c)
Cu(OH)2
d)
correct answer is not given
31.
Chlorine and Flourine will form an ionic bond together since they are in the same group.
a)
True
b)
False
32.
Magnesium and Sulfur would probably be able to form an ionic bond.
a)
True
b)
False
33.
Mg3N2
a)
Magnesium Nitride
b)
Trimanganese dinickel
c)
Magnesium (I) Nitride
34.
How many electrons will sulfur lose or gain when forming an ion?
a)
lose 2
b)
gain 2
c)
gain 6
d)
lose 6
35.
FeBr is called
a)
iron bromine
b)
iron (I) bromine
c)
iron bromide
d)
iron (I) bromide
36.
Calcium Nitride
a)
CaN
b)
Ca3N2
c)
Ca2N3
d)
Ca2N
37.
AlF3
a)
Aluminum (I) fluride
b)
Aluminum (II) fluride
c)
Aluminum (III) fluoride
d)
aluminum fluroide
38.
TiCl2
a)
Tin(I) Chloride
b)
Titanium (I) Chloride
c)
Titanium (II) Chloride
d)
Titanium (I) Chloride
39.
Na2S
a)
Sodium Sulfide
b)
Sodium Sulfate
c)
Sodium Sulfite
d)
Disodium Sulfide
40.
Atoms that lose electrons become...
a)
negatively charged (anion)
b)
postively charged (cation)
c)
remain neutral, no charge
d)
losers
41.
Why are ions charged particles?
a)
The number of electrons does not equal the number of protons.
b)
The number of protons does not equal the number of neutrons.
c)
The number of neutrons does not equal the number of electrons.
d)
The electric charges of the electrons and protons cancel each other out.
42.
Which of the following is NOT a characteristic of IONIC COMPOUNDS?
a)
High melting point
b)
Conducts electricity
c)
Strong bonds
d)
Low boiling points
43.
Which two elements could form an ionic compound?
a)
#6 carbon and #8 oxygen
b)
#1 hydrogen and #7 nitrogen
c)
#3 lithium and #9 fluorine
d)
#5 boron and #10 neon
44.
Which of the following compounds is not an ionic compound?
a)
barium oxide
b)
lithium oxide
c)
carbon dixoide
d)
calcium chloride
45.
Which statement about energy and ionic bonds is true?
a)
It takes energy to form a negative ion.
b)
Halogens need the most energy to become ions.
c)
It takes energy to remove valence electrons from an atom.
d)
It takes more energy to gain two electrons than one.
46.
In which of the following elements is the valence electron farthest from the nucleus?
a)
#3 lithium
b)
#11 sodium
c)
#19 potassium
d)
#37 rubidium
47.
What is the chemical name for NH4Cl?
a)
Nitrogen Hydrogen Chloride
b)
Nitrogen Tetrahydrogen Chloride
c)
Ammonium Chloride
d)
Ammounium Calcide
48.
What is the name for Al(CN)3?
a)
Aluminum Cyanide
b)
Aluminum Carbon Nitrogen
c)
Aluminum Tricarbon trinitride
d)
Aluminum Tricarbonitride
49.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
50.
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.
51.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
52.
In general, what can be said of the melting points of metals?
a)
They are low.
b)
They are high.
c)
They are lower than nonmetals.
d)
They do not have melting points.
53.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
54.
Why are alloys generally used to make everyday objects?
a)
Alloys are often stronger and less active than pure metals.
b)
Alloys have higher melting point than pure metals.
c)
Alloys are less expensive to produce than pure metals.
d)
Alloys have ionic bonds instead of metallic bonds.
55.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
56.
acetate
a)
C2H3O21-
b)
C3H2O31-
c)
C2H2O31-
d)
C3H3O21-
57.
phosphate
a)
PO32-
b)
PO33-
c)
PO42-
d)
PO43-
58.
chlorate
a)
ClO21-
b)
ClO31-
c)
ClO41-
d)
ClO1-
59.
cyanide
a)
CN2-
b)
CN1-
c)
CN21-
d)
CNO1-
60.
ammonium
a)
NH41+
b)
NH42+
c)
NH31+
d)
NH32+
61.
nitrite
a)
N3-
b)
NO21-
c)
NO31-
d)
N2O1-
62.
Alloys include a "sea" of free moving _______.
a)
electrons
b)
atoms
c)
molecules
d)
protons
63.
Which is true about ionic bond formation?
a)
It is exothermic which releases heat, and energy of products is lower that reactants.
b)
It is endothermic which releases heat, and energy of products is lower that reactants.
c)
It is exothermic which absorbs heat, and energy of products is lower that reactants.
d)
It is exothermic which releases heat, and energy of products is higher that reactants.
64.
When distance increases, electrostatic force ____________; we call this relationship ____________ proportional
a)
decreases;directly
b)
decreases;inversely
c)
increases;inversely
d)
increases;directly
65.
If the charges on both ions doubles, what happens to the attractive force between the particles?
a)
Quadruples
b)
Doubles
c)
Stays the same
d)
Reduced by half
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