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Periodic Trends and Ionic Bonding

Total questions: 209

Worksheet time: 7hrs 52mins

Name
Class
Date
1.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

2.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

3.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
4.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
5.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
6.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
7.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
8.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
9.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
10.

As you move down a group on 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 neutrons

11.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
12.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
13.
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
14.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
15.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
16.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
17.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
18.
Which of these is a property of metals?
a)
It's malleable
b)
It can't conduct electricity
c)
They are used in food
d)
It's very brittle
19.
If a material can easily be drawn into the shape of a wire, it is
a)
Ductile
b)
Magnetic
c)
Malleable
d)
Reactive
20.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
21.
Which of the following refers to the element that is usually a gas or a brittle solid at room temperature.  It is a poor conductor of heat and electricity.
a)
A. Metals
b)
B. Nonmetals
c)
C. Metalloids
22.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

23.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

24.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
25.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
26.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
27.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
28.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
29.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
30.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
31.

As you move down a group on 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 neutrons

32.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
33.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
34.
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
35.

Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the least ionization energy and electronegativity?

a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
36.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
37.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)

sodium

d)
cesium
38.
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.
39.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
40.
The distance between the nucleus of an atom and the outer edge of the electron cloud
a)
Atomic radius
b)
Ionic Radius
c)
Ionization Energy
d)
Electronegativity
41.
Valence electrons are: 
a)
Electrons in the highest energy level
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons that are excited
42.
A anion will be a ____ ion.
a)
negative
b)
positive
43.
A cation is a ____ ion.
a)
negative
b)
positive
44.
The minimum energy required to remove an electron from the ground state of an atom
a)
electronegativity
b)
electron affinity
c)
ionization energy
d)
reactivity
45.
The tendency of an atom to attract electrons
a)
electronegativity
b)
ionization energy
c)
electron affinity
d)
reactivity
46.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
47.
Put the following elements in order of decreasing ionization energy:
O, Te, Po, S.
a)
O, S, Po, Te
b)
O, S, Te, Po
c)
O, Te, Po, S
d)
O, Po, Te, S
48.
Which is larger:
Ca or Ca2+
a)
Ca
b)

Ca2+

c)
both are same size
d)
impossible to determine
49.

Which is larger:
Mg or Mg2+

a)

Mg

b)

Mg2+

c)
both are same size
d)
impossible to determine
50.
Which of the following would require the most energy to remove an electron?
a)
Sodium
b)
Potassium
c)
Rubidium
d)
Cesium
51.
Which of the following elements has the GREATEST electronegativity?
a)
Cl
b)
As
c)
Zn
d)
Na
52.
As one proceeds from fluorine to iodine in the Halogen family, the electronegativity ____.
a)
Decreases and atomic radius increases
b)
Decreases and atomic radius decreases
c)
Increase and atomic radius increases
d)
Increases and atomic radius decreases
53.
Put the following in order of increasing ionization energy:Tellurium, Sulfur, Selenium
a)
Tellurium, Sulfur, Selenium
b)
Selenium, Sulfur, Tellurium
c)
Sulfur, Selenium, Tellurium
d)
Tellurium, Selenium, Sulfur
54.
Put these in order of increasing electronegativity:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
55.
Which of the following choices is true?
a)
Metals and nonmetals display the same trends of reactivity.  They each increase to the left and down.
b)
Metal reactivity increases to the left and down, while nonmetal reactivity increases to the right and up
c)
Metal reactivity decreases to the left and down, while nonmetal reactivity decreases to the right and up
d)
Metals and nonmetals display the same trends of reactivity.  They each decrease to the left and down.
56.
Why is potassium more reactive than sodium?
a)
Potassium is not more reactive than sodium
b)
Potassium has a lower ionization energy than sodium
c)
Potassium has a higher ionization energy than sodium
57.
Why is potassium more reactive than calcium?
a)
Potassium is not more reactive than calcium
b)
Potassium has 1 valence electron while calcium has 2
c)
Calcium has 1 valence electron while potassium has 2
58.
Which statement is true?
a)
Cl has a higher electronegativity than Ar because it is farther to the left
b)
Ar has a higher electronegativity than Cl because it is farther to the right
c)
Ar does not have an electronegativity value because it has 8 valence electrons
59.
Why is I more reactive than Te?
a)
I has a higher electronegativity
b)
Te has a higher electronegativity
c)
I is not more reactive than Te
60.
Which statement is true?
a)
Ionic radius and atomic radius have the same trend
b)
Ionic radius and atomic radius have an opposite trend
c)
Ionic radius and atomic radius have the same trend except that anions are bigger than cations on the same period
d)
Ionic radius and atomic radius have the same trend except that cations are bigger than anions on the same period
61.

Using the periodic table, the group of the element tells you how many ____________ an element has.

a)

Valence electrons

b)

Protons

62.
The elements on the left side of the periodic table are generally always ______ and the elements on the right side of the periodic table are generally always ______.
a)
cations; anions
b)
anions; cations
c)
reactive; non-reactive
d)
non-reactive; reactive
63.

Which of the following diagram representing sodium chloride is/are correct? (You can choose more than 1 answer)

a)

b)

c)

None of them

64.

In an ionic bond, ​ (a)   transfer from the ​ (b)   to the ​ (c)   .

Choose from the below words
electron(s)
metal
non-metal
65.

Mg and Br

(a)  

66.

Al and O

(a)  

67.

Li and O

(a)  

68.

Sr and F

(a)  

69.

Na and P

(a)  

70.

Mg and S

(a)  

71.

Ca and N

(a)  

72.

K and Se

(a)  

73.

Be and N

(a)  

74.

Ba and I

(a)  

75.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
76.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
77.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
78.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
79.
Which of the following element is most likely to form an ion with a 2+ charge?
a)
calcium (Ca)
b)
potassium (K)
c)
carbon (C)
d)
fluorine (F)
80.

Which of the following element is most likely to form an ion with a 1+ charge?

a)
calcium (Ca)
b)
potassium (K)
c)
carbon (C)
d)
fluorine (F)
81.

Which of the following element is most likely to form an ion with a 1- charge?

a)
calcium (Ca)
b)
potassium (K)
c)
carbon (C)
d)
fluorine (F)
82.

Which of the following element is most likely to form an ion with a 2- charge?

a)
calcium (Ca)
b)
potassium (K)
c)

Oxygen (O)

d)
fluorine (F)
83.

Which of the following element is most likely to form an ion with a 3- charge?

a)

aluminum (Al)

b)

phosphorus (P)

c)

oxygen (O)

d)
fluorine (F)
84.

Which of the following element is most likely to form an ion with a 3+ charge?

a)

aluminum (Al)

b)

phosphorus (P)

c)

oxygen (O)

d)
fluorine (F)
85.

Which of the following element is most likely to form an ion with a 1- charge?

a)
calcium (Ca)
b)
potassium (K)
c)
carbon (C)
d)
fluorine (F)
86.
LiBr is called
a)
lithium bromine
b)
lithium (I) bromine
c)
lithium bromide
d)
lithuim (I) bromide
87.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
88.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
89.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
90.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
91.
What formula results when Ca+2 and Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
92.
The chemical formula of potassium iodide is
a)
KI
b)
PI
c)
KI₂
d)
K₂I
93.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
94.
charged particle; has either more or fewer electrons than protons
a)
Chemical Bond
b)
chemical formula
c)
covalent bond
d)
ion
e)
ionic bond
95.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
96.
Which is most likely to form a negative ion...
a)
an element from Group 17
b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
97.
Which of the following is the correct name for MgCl2....
a)
Magnesium Clorine
b)
Magnesium Dicholorine
c)
Magnesium Cloride
d)
Magnesium Dichloride
98.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
99.
The attraction between oppositely charged ions is called a(n) _______________.
a)
ionic bond
b)
polyatomic ion
100.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
101.
In order to have a stable arrangement of 8 valence electrons, metal atoms are likely to _________electrons.
a)
gain
b)
lose
102.
In an ionic compound, the total positive charge of all the positive ions ___________ the total negative charge of all the negative ions.
a)
equals
b)
is more than
103.
Because the force of attraction between the positive and negative ions is so strong, ionic compounds have _________ melting points.
a)
high
b)
low
104.

Using the periodic table, the group of the element tells you how many ____________ an element has.

a)

Valence electrons

b)

Protons

105.
The elements on the left side of the periodic table are generally always ______ and the elements on the right side of the periodic table are generally always ______.
a)
cations; anions
b)
anions; cations
c)
reactive; non-reactive
d)
non-reactive; reactive
106.

Which of the following diagram representing sodium chloride is/are correct? (You can choose more than 1 answer)

a)

b)

c)

None of them

107.

In an ionic bond, ​ (a)   transfer from the ​ (b)   to the ​ (c)   .

Choose from the below words
electron(s)
metal
non-metal
108.

Where are metals located on the periodic table?

a)

Blue

b)

Orange

c)

Yellow

d)

Red

109.

Ionic Bonds

a)

Non metal and non metal

b)

Metal and non metal

110.

The positive ions tend to _____________ electrons.

a)

Share

b)

Lose

c)

Gain

d)

Neutral

111.

Where are the metalloids located on the periodic table? 

a)

Blue

b)

Green

c)

Orange

d)

Red

112.

Ionic bonds form between two ions that have...

a)

Positive Chargers

b)

negative charges

c)

Same Charges

d)

Opposite Charges

113.

How does calcium become a calcium ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

114.

How does oxygen become an oxide ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

115.

An electron has what kind of charge?

a)

equal charge

b)

no charge

c)

negative charge

d)

positive charge

116.

What is the ionic compound that is formed when you combine Li+ and N-3 ions?

a)

LiN

b)

LiN3

c)

Li3N2

d)

Li3N

117.

Is hydrogen considered a metal or a non-metal or metalloid

a)

non-metal

b)

metal

c)

metalloid

118.

What does the 6 represent?

a)

Atomic mass

b)

Atomic number

c)

Isotope

d)

Atomic Symbol

119.

Electrons located on the outermost shell are called _________ electrons

a)

Hybrid

b)

Atomic

c)

Neutral

d)

Valence

120.

Atoms form bonds with other atoms in order to be ______

a)

Happy

b)

Stable

c)

Not Happy

d)

Friends

121.

The valence shell corresponds to this grouping on the periodic table?

a)

The Groups

b)

The Periods

c)

Ionic compounds

d)

Molecular compounds

122.

Which of the following elements has the highest ionization energy?

a)

Helium

b)

Hydrogen

c)

Lithium

d)

Beryllium

123.

Which of the following elements is a metalloid?

a)

Silicon

b)

Oxygen

c)

Aluminum

d)

Iron

124.

Which of the following elements has the smallest atomic radius?

a)

Hydrogen

b)

Helium

c)

Lithium

d)

Beryllium

125.

Which of the following elements has the highest electronegativity?

a)

Oxygen (O)

b)

Fluorine (F)

c)

Nitrogen (N)

d)

Carbon (C)

126.

Which of the following elements has the lowest electronegativity?

a)

Oxygen (O)

b)

Fluorine (F)

c)

Nitrogen (N)

d)

Carbon (C)

127.

As you move from left to right across a period in the periodic table, the atomic radius generally...

a)

increases

b)

decreases

c)

remains the same

d)

alternates between increasing and decreasing

128.

As you move from right to left across a period in the periodic table, the atomic radius generally...

a)

increases

b)

decreases

c)

remains the same

d)

alternates between increasing and decreasing

129.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
130.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
131.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
132.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
133.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
134.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
135.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
136.
Which of the following has a -1 charge? 
a)
Aluminum
b)
Bromine
c)
Calcium
d)
Potassium
137.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
138.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
139.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
140.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
141.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
142.
What is the ionic symbol for a Caesium atom?
a)
Cs+
b)
Cs-
c)
Cs+2
d)
Cs-2
143.
Make sure you get enough Potassium in your diet!
a)
Huh?
b)
K
c)
I <3 bananas
d)
Sure
144.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

145.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

146.

What type of atom is this?

a)

Neutral atom

b)

Cation

c)

Anion

d)

Isotope

147.

What two particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

148.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

149.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
150.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

151.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

152.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

153.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

154.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

155.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

156.

Sodium (Na) has 1 electron (e-) in its outer shell (orbital). How can it make a full outer shell? (HINT: Think of which option would be "easier" for the atom.)

a)

Giving away or donating the outer electron.

b)

Taking on or accepting 7 more electrons.

157.

Knowledge Check:

Why does Sodium become a +1 charge?

a)

Sodium gives away 1 e-, so it now has 1 less negative (-) charge.

b)

Sodium accepts 1 e-, so it now has 1 more negative (-) charge.

158.

Knowledge Check:

Why does Chlorine (Cl) become a -1 charge?

a)

Cl donates an e-, so it now has 1 less negative (-) charge.

b)

Cl accepts an e-, so it now has 1 more negative (-) charge.

159.

What is a anion?

a)

a neutral ion

b)

an atom with a negative charge

c)

and atom with a positive charge

d)

an atom that has lost electrons

e)

an atom that has gained electrons

160.

What class of elements tends to lose electrons?

a)

metals

b)

nonmetals

c)

metalloids

d)

Noble Gas

161.

What class of elements tends to gain electrons?

a)

metals

b)

nonmetals

c)

metalloids

d)

Noble Gas

162.

When an atom gains a valence electron, it becomes a(n) _____________ ion.

a)

positive

b)

negative

c)

neutral

163.

When an atom loses a valence electron, it becomes a(n) _____________ ion.

a)

positive

b)

negative

c)

neutral

164.

Match the charge with the groups.

a)

-1

1.

Group 17

b)

-3

2.

Group 15

c)

-2

3.

Group 16

165.

Match the charge with the groups.

a)

+1

1.

Group 1

b)

+2

2.

Group 2

c)

+3

3.

Group 3

166.
anions are _____ ions.
a)
positive
b)
negative
c)
neutral
167.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
168.
What charge will a sulfide ion have?
a)
3+
b)
2+
c)
2-
d)
3-
169.
What charge will a nitride ion have?
a)
3+
b)
2+
c)
2-
d)
3-
170.
what charge will an aluminum ion have?
a)
3+
b)
2+
c)
2-
d)
3-
171.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
172.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
173.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
174.
How many valence electrons does Sulfur
a)
16
b)
32
c)
6
d)
3
175.
How many valence electrons does Krypton have?
a)
36
b)
18
c)
8
d)
4
176.
If an atom has 3 valence electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
177.
If an element gains 1 electron, what charge will it have?
a)
+1
b)
-1
c)
+7
d)
-7
178.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
179.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
180.
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.
181.
anions are _____ ions.
a)
positive
b)
negative
c)
neutral
182.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
183.
What charge will a sulfide ion have?
a)
3+
b)
2+
c)
2-
d)
3-
184.
What charge will a nitride ion have?
a)
3+
b)
2+
c)
2-
d)
3-
185.
what charge will an aluminum ion have?
a)
3+
b)
2+
c)
2-
d)
3-
186.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
187.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
188.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
189.
How many valence electrons does Sulfur
a)
16
b)
32
c)
6
d)
3
190.
How many valence electrons does Krypton have?
a)
36
b)
18
c)
8
d)
4
191.
If an atom has 3 valence electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
192.
If an element gains 1 electron, what charge will it have?
a)
+1
b)
-1
c)
+7
d)
-7
193.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
194.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
195.
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.
196.
anions are _____ ions.
a)
positive
b)
negative
c)
neutral
197.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
198.
What charge will a sulfide ion have?
a)
3+
b)
2+
c)
2-
d)
3-
199.
What charge will a nitride ion have?
a)
3+
b)
2+
c)
2-
d)
3-
200.
what charge will an aluminum ion have?
a)
3+
b)
2+
c)
2-
d)
3-
201.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
202.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
203.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
204.
How many valence electrons does Sulfur
a)
16
b)
32
c)
6
d)
3
205.
How many valence electrons does Krypton have?
a)
36
b)
18
c)
8
d)
4
206.
If an atom has 3 valence electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
207.
If an element gains 1 electron, what charge will it have?
a)
+1
b)
-1
c)
+7
d)
-7
208.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
209.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2