Free Printable Ionic and Covalent Review

Worksheets

Ionic and Covalent Review

Total questions: 70

Worksheet time: 1hrs 12mins

Name

Class

Date

What is the correct name for NaClO?

Sodium hypochlorite

Sodium chlorite

Sodium chlorate

Sodium perchlorate

Which is the correctly balanced ionic compound for aluminum oxide?

$AlO$

$Al^2O^3$

$Al_2O_3$

$Al_3O_2$

Which ion is named first in an ionic compound?

Anion

Cation

The largest

The most electronegative

For a compound formed with a polyatomic ion, which name is used?

The names of all elements in the polyatomic ion

The name of the most abundant element

The name of the most reactive element

The name of the polyatomic ion

What is wrong with the ionic compound $NaS_2$ ?

Charges not properly balanced

No positive charge

No negative charge

What is the correct name for $HgCl_2$ ?

Mercury chloride

Mercury (II) chloride

Mercury chlorite

Mercury (II) chlorite

What is the correct name for CaO?

Calcium oxide

Calcium oxite

Calcium oxygen

Calcide oxygen

What is the correct name for $NH_4OH$ ?

Nitrogen hydrogen oxygen

Nitride hydroxide

Ammonia hydroxide

Ammonium hydroxide

What is the correct name for $Na_2CrO_4$ ?

Disodium chromate

Sodium chromium oxygen

Sodium chromate

Sodium chromoxide

10.

What is the correct ionic formula for zinc sulfide?

$ZnS$

$ZNS$

$ZnS_2$

$ZnSO_4$

11.

What is the correct formula for silver nitrite?

$AgNO_3$

$AgNO_2$

$AgNO$

$AgN$

12.

What is the correct ionic formula for strontium phosphate?

$SrPO_3$

$SrPO_4$

$Sr_3\left(PO_3\right)_2$

$Sr_3\left(PO_4\right)_2$

13.

What is the correct ionic formula for potassium nitride?

$KN$

$KN_3$

$K_3N$

14.

An ionic compound forms between a _______ and _______.

metal and non-metal

two metals

two non-metals

15.

Name the ionic compound, LiCl

lithium chlorine

lithium chloride

lithium chlorate

lithium monochloride

16.

Name the molecular compound CO

carbon monoxide

monocarbon monoxide

carbide

oxygen carbide

17.

K₂0 - name?

potassium dioxide

potassium oxide

potassium oxygen

dipotassium dioxide

18.

Where are the non-metals located on the periodic table?

All over

On the left side of the "staircase"

On the right side of the "staircase"

19.

Ba(ClO₃)₂ name?

barium chlorate

barium chloride

chlorine bariate

chlorine baride

20.

Give the formula for oxygen dichloride

OCl₂

O₂Cl₂

OCl

O₂Cl

21.

How many valence electrons does nitrogen have?

22.

What part of an atom is involved in chemical bonding?

protons

neutrons

electrons

nucleus

23.

A covalent bond involves a __________ of electrons.

sharing

borrowing

exchanging

switching

24.

A __________ is a number written to the right of a chemical symbol and slightly below it.

subscript

coefficient

chemical formula

compound

25.

What is the chemical formula for Tetrasulfur pentoxide?

S₄O

S₄O₅

S₅O₄

26.

What is the name of C₃Cl₈?

Carbon octachloride

Tricarbon octachloride

Carbon trichloride

Octacarbon trichloride

27.

What kind of compound rarely dissolves in water?

Ionic Compounds

Covalent Compounds

Acids

Bases

28.

lead (II) phosphate

PbPO₄

Pb₂PO₄

Pb₃(PO₄)₂

Pb2(PO₄)₃

29.

If CbO₄^-2 is Cribbite, what is the formula for Cribbate?

CbO₃^-2

CbO₂^-2

CbO₅^-2

CbO₅^-1

30.

A(n) _________ is an ion with a negative (-) charge.

anion

ion

cation

solute

31.

Which of the following is NOT a characteristic of IONIC COMPOUNDS?

High melting point

Conducts electricity

Strong bonds

Low boiling points

32.

___________ is the tendency of an atom to attract (pull) electrons away from other atoms.

Electronegativity

Octet rule

Solubility

Conductivity

33.

Beryllium and sulfur will form a ______ bond

ionic

covalent

metalloid

34.

Nitrogen and Oxygen will make a ____________ bond

ionic

covalent

metallic

35.

How many valence electrons does oxygen have?

36.

hexaboron monosilicide

B₆Si

BSi

BSi₆

B₆Si₆

37.

What is the correct structure for BF₃?

Option A.

Option B.

Option C.

Option D.

38.

When writing Lewis Structures, only __________ electrons are used.

Inner shell

Core

Valence

Stable

39.

Each line in a Lewis Structure represents __________ electron(s).

40.

VSEPR theory is used to predict

the number of unshared pairs of electrons in a Lewis structure.

the number of multiple bonds in a Lewis structure.

the three-dimensional geometry of a molecule.

the three-dimensional crystal lattice structure of ionic compounds.

41.

Choose the correct shape for this molecule:

Trigonal planar

Trigonal pyramidal

Bent

Tetrahedral

42.

How many electrons does hydrogen need to have a full octet?

43.

If an element forms a suboctet, which of the below statements are TRUE?

It appears before period 3 in the periodic table.

It does not require 8 electrons to have a full octet.

It can accept additional electrons in a coordinate covalent bond.

All of these answers are true.

44.

If an elements forms an expanded octet,

It is happy with less than 8 electrons.

It is happy with only 2 electrons.

It will accept more than 8 electrons.

None of these.

45.

Between the molecule on the left and right, which C-N bond has the greatest bond-dissociation energy?

Left

Right

46.

Which option illustrates the steps for determining a Lewis structure shown in the correct order?

Determine the total number of valence electrons, draw multiple bonds, add lone pairs to the central atom

Draw electrons around central atom, draw electrons around terminal ends, double-check all octets

Draw electrons around terminal ends, determine the total number of valence electrons, steal lone pairs to form multiple bonds

Determine the total number of valence electrons, draw a single bond from all terminal ends to the central atom, double-check all octets

47.

What shape does this have?

Tetrahedral

Trigonal pyramidal

Trigonal bipyramidal

Astrahedral

48.

TRUE OR FALSE: The element farthest to the left or down on the periodic table is the most electronegative.

True

False

49.

The shared electron pair is closer to one end than the other in a ________________ molecule.

Polar

Nonpolar

Ionic

Covalent

50.

Which bond is the most polar?

C-O

Si-O

C-Cl

C-Br

51.

When metal atoms form ions, do they lose or gain electrons?

Lose

Gain

52.

Which type of bonding is between a metal and a non-metal?

covalent

ionic

metallic

53.

Which type of bonding is found in sodium chloride?

Ionic

Covalent

metallic

54.

When would you find covalent bonding?

Between metal and non-metal

In metals

Between two or more non-metals

55.

Why do metals and ionic compounds have high melting and boiling points?

Because of the strong electrostatic forces of attraction

Because of the strong covalent bonds

Because of the weak intermolecular forces

56.

What are giant ionic substances in a regular arrangement called?

lattice

molecular

grid

57.