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Periodic Trends and Ionic Bonding

Total questions: 26

Worksheet time: 43mins

Name
Class
Date
1.

The anion form of an atom is always _______ than its neutral form.

a)

smaller

b)

larger

c)

the same

d)

unable to tell

2.

The cation form of an atom is always ________ than its neutral form.

a)

smaller

b)

larger

c)

the same

d)

unable to tell

3.

The ____ of an atom is found by measuring the distance between the nuclei of two like atoms and halving that distance.

a)

Electronegativity

b)

Atomic Radius

c)

Ionic Size

d)

Ionization Energy

4.

Which of the following elements does not want to have 8 valence electrons?

a)

Mg

b)

O

c)

H

d)

N

5.

An ionic compound

a)

composed of anions and cations

b)

held together by ionic bonds

c)

composed of metals and non metals

d)

all of these

6.

Ionic compounds are normally in which physical state at room temperature?

a)

gas

b)

solid

c)

liquid

d)

plasma

7.

Which of the following is NOT a characteristic of Ionic compounds

a)

the have low melting points

b)

they are composed of a metal and a non metal

c)

they are solids

d)

they conduct electricity in liquid form

8.

How many electrons does a nitrogen atom need to gain to attain a complete octet?

a)

5

b)

4

c)

3

d)

2

9.

Which of the following pairs of elements is most likely to form an ionic compound?

a)

Mg and Na

b)

N and S

c)

O and Cl

d)

Mg and Cl

10.

Match the following

a)

Atomic Number

1.

The periodic table is organized by this

b)

Alkaline Earth Metal

2.

Name for group 2 elements

c)

Halogens

3.

The elements in group 17 are called

d)

Transition Metals

4.

Name for group 3-12 elements

11.

Match the following

a)

Ductile

1.

Metals that can be made into wire

b)

Electronegativity

2.

Elements attractiveness to electrons

c)

Mendeleev

3.

Arranged the periodic table

d)

Ionic Bonding

4.

transfer of electrons

e)

aqueous

5.

means dissolved in water

12.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

13.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

14.
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
15.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
16.
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
17.

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

18.

What makes the noble gases unique?

a)

They're the only gases on the periodic table.

b)

They have a full valence shell.

c)

Nothing else on the periodic table has that name.

d)

They have an empty valence shell.

19.

An "ionic bond" is named that way because ions are formed from the gaining/losing of electrons between metals and non-metals.  Which of the following is NOT an ionic compound?

a)

Li2OLi_2O  

b)

CO2CO_2  

c)

CaSCaS  

d)

CaCl2CaCl_2  

20.

Which of these forms an ionic bond?

a)

Na and Cl

b)

C and O

21.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
22.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

23.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

24.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
25.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
26.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.

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