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Pre UPS 1 DK014

Total questions: 50

Worksheet time: 13hrs 30mins

Name
Class
Date
1.

What is matter?

a)

anything that has mass and takes up space

b)

anything that can be felt

c)

anything that can behave in many different ways

d)

anything that exist on Earth

2.
A mixture that appears to be evenly mixed throughout is ___________________.
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
3.
I am 2 or more elements chemically combined.
a)
atom
b)
molecule
c)
compound
d)
mixture
4.
A mixture that does NOT appear to be evenly mixed throughout is ____________________.
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
5.

Which of these is an element?

a)

Salt (NaCl)

b)

Water (H20)

c)

Oxygen (O)

d)

Carbon Dioxide (CO2)

6.

Which of these is a compound?

a)

Aluminium (Al)

b)

Carbon Dioxide (CO2)

c)

Nitrogen (N)

d)

Sand

7.
Which of the following is a pure substance? 
a)
Water
b)
Salad
c)
Chocolate milk
d)
All of them 
8.

An element

a)

contains one type of atom

b)

contains two or more different type of atoms

c)

is two or more different substances not chemically combined

d)

is the way something is put together or combined

9.

Contains two or more different substances that are physically, not chemically, combined

a)

a mixture

b)

an element

c)

a compound

d)

a chemical formula

10.
What does this picture represent?
a)
solid
b)
liquid
c)
gas
d)
plasma
11.
What does this picture represent? 
a)
solid
b)
liquid
c)
gas
d)
plasma
12.
What does this picture represent? 
a)
solid
b)
liquid 
c)
gas
d)
plasma
13.
Which of the following is not true about gases?
a)
They spread out to fill their containers
b)
They have a low density. 
c)
The particles move very slowly. 
d)
The volume changes with whatever shape the room is. 
14.
Which is true about solids?
a)
They particles can move past each other. 
b)
The particles vibrate in their positions. 
c)
The particles do not form a pattern. 
d)
Solids have the highest kinetic energy
15.
Which phase has a constant volume and a constant shape? 
a)
solid
b)
liquid
c)
gas
d)
plasma
16.
The steam coming off the pot of boiling water is an example of....
a)
a solid becoming a liquid
b)
a liquid becoming a solid
c)
a liquid becoming a gas
d)
a gas becoming a liquid
17.
Which of the following statements is NOT true of all different types of matter?
a)
They are made of atoms and molecules
b)
The particles are always in motion
c)
The particles always move at the same speed
d)
They are made of particles that are too small to see
18.
Change of state from a solid directly to a gas is called
a)
deposition
b)
melting
c)
evaporation
d)
sublimation
19.
Found in the nucleus of the atom
a)
electrons only
b)
protons only
c)
neutrons and protons
d)
neutrons and electrons
20.
Atomic number=
a)
number of neutrons
b)
atomic mass
c)
protons
d)
electrons+protons
21.
Mass Number is--
a)
the number of protons + neutrons
b)
the number of protons
c)
the number of electrons +protons +electrons
d)
the same as atomic number
22.
The bottom number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
23.

The upper number in this isotope notation represent

a)

the nucleon number

b)

the proton number

c)

the element symbol

d)

the neutron number

24.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
25.
The photo above shows the isotopic notation for which isotope?
a)
Carbon 12
b)
Carbon 13
c)
Carbon 14
d)
Carbon 15
26.

How many neutrons does an atom of the isotope Neon-22 have if its proton number is 10?

a)

12

b)

10

c)

22

d)

20

27.

How many protons, neutrons and electrons are in the neutral atom of Cl 17

35 ?

a)

A. 17 protons, 15 neutrons and 17 electrons

b)

B. 17 protons, 17 neutrons and 17 electrons

c)

C. 17 protons, 17 neutrons and 18 electrons

d)

D. 17 protons, 18 neutrons and 17 electrons

28.

What is the mass number of the element shown?

a)

15

b)

7

c)

8

d)

0

29.
Atoms of the same element but with different numbers of neutrons.
a)
Ion
b)
Isotope
c)
Mass Number
d)
electron
30.

The diagram shows three isotopes of hydrogen element. The heaviest isotope of hydrogen has

a)

three shells

b)

three protons

c)

two neutrons

d)

one electron

31.

An atom of an element is electrically neutral because the number of protons

is equal to the number of _____________.

a)

A. electrons

b)

B. neutrons

c)

C. nucleons

d)

D. nucleus

32.

How do we call the protons and neutrons that are found together in the

nucleus?

a)

A. nuclei

b)

B. nucleons

c)

C. atomic mass

d)

D. mass number

33.

Oxidation number of O in its stable elemental form, O2:

a)

0

b)

-1

c)

-2

d)

+2

34.

Oxidation number of O in the compound H2O2:

a)

0

b)

-1

c)

-2

d)

+2

35.

Oxidation number of O in the ion H3O+:

a)

0

b)

-1

c)

-2

d)

+2

36.

Oxidation number of H in NaH:

a)

0

b)

+1

c)

-1

d)

+2

37.

C in CO32-?

a)

-4

b)

+2

c)

0

d)

+4

38.
Determine the number of
atoms in
2.50 moles of zinc.
a)
1.51 x 1024 atoms
b)
4.15 x 10-24 atoms
c)
2.71 x 10-22 atoms
d)
163 atoms
39.
A mole of carbon dioxide contains 6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
40.
How many moles are 98.3 grams of aluminum hydroxide, Al(OH)3?
a)
1.26 moles
b)
0.8 moles
c)
7,673.4 moles
d)
150 moles
41.

Convert 25 g of NaBr to molecules

a)

102.96 molecules

b)

0.24 molecules

c)

1.45x1023 molecules

d)

2.34 x 1020molecules

42.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
43.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
44.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
45.

Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.

a)

2.18 M

b)

0.746 M

c)

1.18 M

d)

0.545 M

46.

What is the molarity of a solution of nitric acid that contains 12.6 grams nitric acid in 1.2 L of solution?

a)

0.167 M

b)

0.538 M

c)

0.378 M

d)

0.812 M

47.

This is the formula used to determine

a)

percentage by mass

b)

percentage by volume

c)

molarity

d)

mole fraction

48.

A solution is prepared by dissolving 0.60 g of sodium chloride NaCl in 500 mL of water. Identify the solute.

a)

water

b)

sodium chloride

c)

NaCl solution

d)

distilled water

49.

Calculate the percentage by mass of solution, if there is 100 g of sugar and 400 g of water

a)

30

b)

25

c)

20

d)

15

50.

The density of 80% by mass of sulphuric acid, H2SO4 solution is 1.73 g mL–1. Calculate the molarity of the acid solution.

a)

7.05 molL-1

b)

14.1 molL-1

c)

28.2 molL-1

d)

10.0 molL-1

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