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MYP Chemistry unit review

Total questions: 80

Worksheet time: 1hrs 21mins

Name
Class
Date
1.
Which of the following is described as the basic unit of matter?
a)
Element
b)
Atom
c)
Molecule
d)
Compound
2.

Which of the following techniques can we use to separate homogeneous mixtures?

a)

Crystallisation

b)

Distillation

c)

Evaporation

d)

All of the above

3.

Name the separation technique

a)

Centrifuge

b)

Bunsen burner

c)

Distillation

d)

Evaporation

4.

Name the separation technique

a)

Distillation

b)

Crystallisation

c)

Magnetic Separation

d)

Condensation

5.

Name the separation technique

a)

Filtration

b)

Evaporation

c)

Distillation

d)

Separation

6.

In a salt water solution ...

a)

Salt is the solute and water is the solvent

b)

Salt is the solvent and water is the solute

7.

Which of the following statements tells us that a sample of liquid is pure water?

a)

It is colourless.

b)

It leaves no residue when filtered.

c)

It boils at 100oC.

d)

It is odourless.

8.

What is the name of this separation technique?

a)

distillation

b)

filtration

c)

evaporation

d)

chromatography

9.

For paper chromatography to work,

a)

the dyes must have different boiling points.

b)

the dyes must have different solubilities in the solvent.

c)

the starting line on the chromatogram must be drawn using pen.

d)

The starting line must be below the level of the solvent.

10.

Which ink is most soluble?

a)

Blue

b)

Red

c)

Yellow

d)

Green

11.

Which ink is a mixture?

a)

Blue

b)

Red

c)

Yellow

d)

Black

12.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

13.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

14.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
15.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
16.

Which elements have the most similar chemical properties?

a)

boron and carbon

b)

oxygen and sulfur

c)

aluminum and bromine

d)

argon and silicon

17.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
18.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
19.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

20.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

21.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

22.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

23.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

24.

Two objects that are similarly charged will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

25.

An object becomes positively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

26.

An object becomes negatively charged by...

a)

gaining negative charges.

b)

losing negative charges.

c)

gaining positive charges.

d)

losing positive charged.

27.

Metal atoms are most likely to form...

a)

positively charged cations.

b)

negatively charged anions.

c)

neutral molecules.

d)

bations.

28.

Electrolyte solutions are formed when compounds dissolve and break apart into...

a)

charged particles.

b)

neutral particles.

c)

atoms.

d)

liquid particles.

29.

Non-Metal atoms are most likely to form...

a)

positively charged cations.

b)

negatively charged anions.

c)

neutral molecules.

d)

bations.

30.

Atoms from group 2 on the Periodic Table are likely to form ions of what charge?

a)

+1

b)

+2

c)

0

d)

−1

e)

−2

31.

Atoms from group 16 on the Periodic Table are likely to form ions of what charge?

a)

+1

b)

+2

c)

0

d)

−1

e)

−2

32.

What is the name of an ionic compound formed from Calcium and Oxygen?

a)

Calcium Oxide

b)

Calcium Monoxide

c)

Monocalcium Monoxide.

d)

Calcium Dioxide

33.

What is the formula of an ionic compound formed from Lithium and Oxygen?

a)

Li2O

b)

LiO2

c)

2LiO

d)

Li2O

34.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
35.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
36.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
37.

Which of the following atoms will GAIN electrons to form an ion? (check all that apply)

a)

Calcium

b)

Neon

c)

Bromine

d)

Nitrogen

e)

Rubidium

38.

Which of the following atoms will LOSE electrons to form an ion? (check all that apply)

a)

Calcium

b)

Neon

c)

Bromine

d)

Nitrogen

e)

Rubidium

39.

Beryllium will ________ electrons to form an ion. It's ion symbol is _______.

a)

lose 2; Be2-

b)

lose 2; Be2+

c)

gain 6; Be6-

d)

gain 6; Be6+

40.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
41.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
42.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
43.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
44.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
45.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
46.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
47.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
48.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

49.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

50.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

51.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

52.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

53.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

54.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

55.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

56.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

57.

By looking at the formula of an ionic compound, we can determine the charge (oxidation state) of a transition metal.

a)

True

b)

False

58.
What is the charge on the hydroxide ion?
a)
0
b)
-1
c)
-2
d)
-3
59.

When silver nitrate is added to a solution of Iodide ions what is the expected results ?

a)

Cream precipitate

b)

White precipitate

c)

Yellow precipitate

d)

No visible change

60.

What colour precipitate does barium sulphate form?

a)

White

b)

Green

c)

Yellow

d)

Cream

61.

What is initially observed when sodium hydroxide is added in excess to a solution of Fe2+ ions?

a)

Green precipitate

b)

Brown precipitate

c)

Blue precipitate

d)

White precipitate

62.

A green precipitate formed when sodium hydroxide is added to an unknown solution indicates the presence of.....

a)

Iron(III)

b)

Calcium

c)

Copper

d)

Iron(II)

63.

Dilute sodium hydroxide can be added to an unknown solution to indicate the presence of....

a)

Iron(II)

b)

Iron(III)

c)

Copper

d)

All of them

64.

Which metal produces an apple green flame?

a)

Barium

b)

Calcium

c)

Silver

d)

Lead

65.

Which metal produces a brick red flame?

a)

Barium

b)

Calcium

c)

Silver

d)

Lead

66.

Silver nitrate and nitric acid are used to test for....

a)

Metals

b)

Noble gases

c)

Halogens

d)

Metal oxides

67.

A gas produced when nitric acid is added to an unknown solution indicates the presence of....

a)

Sulfate

b)

Carbonate

c)

Phosphate

d)

Nitrate

68.

In flame testing, what element is indicated by an yellow flame?

a)

Carbon

b)

Sodium

c)

Copper

d)

Lithium

69.

When doing a flame test, what element is indicated by a purple/lilac flame?

a)

Barium

b)

Calcium

c)

Potassium

d)

Copper

70.

Which ion can be detected in solution by adding dilute sodium hydroxide and then warming, before testing the gas given off with damp red litmus paper? A blue colour is a positive result.

a)

Ammonium

b)

Chloride

c)

Sulfate

d)

Carbonate

71.

Many ions can be detected in solution by adding another solution and observing the colour of the solid formed. What term is given to a solid formed in a reaction between two solutions?

a)

Filtrate

b)

Precipitate

c)

Residue

d)

Solution

72.

What is the colour of the solid hydroxide formed when testing for copper(II) ions?

a)

Blue

b)

Green

c)

Orange

d)

Brown

73.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

74.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
75.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

76.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

77.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

78.
The reason that a sodium atom bonds with a chlorine atom is because
a)
Sodium transfers an electron to Chlorine
b)
oppositely charged ions form a strong electrostatic attraction
c)
ions are the same size
d)
the ions have a full outer shell
79.
The sum of the charges on the ions in a unit of the compound is ___________. 
a)
positive
b)
negative
c)
zero
d)
±1
80.

Which is not true of the chemical bond shown on the diagram?

a)

An electron from Na is transferred to Cl.

b)

The bond is ionic since electron is shared by the two atoms.

c)

A metal and a non-metal are involved in the bonding.

d)

Na will become positively charged and Cl will be negatively charged.

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