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semster 1 exam

Total questions: 73

Worksheet time: 50mins

Name
Class
Date
1.
Which of the following is not evidence of a chemical change?
a)
A precipitate being formed
b)
Gas bubbles being produced
c)
Light production
d)
A liquid freezing into a solid
2.
Which of the following is a chemical change?
a)
A glass hiting the floor and breaking
b)
Wrapping paper being torn
c)
A chocolate bar melting in the car on a hot day
d)
A cake being made in the oven.
3.
Which of the following is a physical change?
a)
A bathroom filling up with steam from a hot shower
b)
Toasting toast
c)
Boiling an egg
d)
Fireworks being set of in the sky
4.
A physical change is one in which the substance in not changed at the molecular level.
a)
True
b)
False
5.
Chemical changes result in new products.
a)
True
b)
False
6.
Which of the following is a chemical property?
a)
flammability
b)
color
c)
texture
d)
shape
7.
Which of the following is a physical property?
a)
mass
b)
pH
c)
toxicity
d)
corrosiveness
8.
Density is a intensive property, meaning the amount present does not change the property.
a)
true
b)
false
9.
Which of the following states of matter are the most compressible?
a)
solid
b)
liquid
c)
gas
10.
This state of matter has a fixed volume and shape.
a)
solid
b)
liquid
c)
gas
d)
plasma
11.
Contact solution is a heterogenous mixture because it looks uniform throughout.
a)
True
b)
False
12.
Rows on the periodic table run from side to side.
a)
True
b)
False
13.
Elements in the same vertical group are more similar to each other.
a)
True
b)
False
14.
Chemical reactivity is based on what subatomic particle?
a)
protons
b)
electrons
c)
valence electrons
d)
neutrons
15.
The identity of an atom can always be determined by the number of ______________ it has.
a)
protons
b)
electrons
c)
valence electrons
d)
neutrons
16.
Electrons are ________ charged and found in the __________.
a)
positively, nucleus
b)
positively, electron cloud
c)
negatively, electron cloud
d)
negatively, nucleus
17.
Mendeleev arranged his table by increasing atomic ________, but Mosely put it in order by increasing atomic _________.
a)
mass, number
b)
number, mass
c)
particles, moles
d)
moles, particles
18.
Groups 1 and 17 are the most reactive elements are are called______________ &______________ respectively.
a)
alkaline earth metals & noble gases
b)
noble gases & transition metals
c)
alkali metals & halogens
d)
lanthanides and actinides
19.
Noble gases are unreactive because
a)
They have a full outer shell
b)
They are positively charged
c)
Gases cannot react
d)
The neutrons are equal to their protons
20.
Which of the following is a property of nonmetals?
a)
ductility
b)
brittleness
c)
malleability
d)
high luster
21.
When electrons are removed, the atoms becomes a positively charged
a)
cation
b)
anion
c)
binary
d)
polyploid
22.
Which of the following elements is this a Bohr's model for?
a)
Carbon
b)
Lithium
c)
Sodium
d)
Magnesium
23.
Using the Gold Foil experiment, Rutherford learned about this positively charged particle.
a)
electron
b)
neutron
c)
proton
24.
If an element has an atomic number of 11 and a mass of 23, how many neutrons does it have?
a)
11
b)
23
c)
12
d)
34
25.
The electron configuration for Sulfur would end in what block?
a)
s
b)
p
c)
d
d)
f
26.
The Noble Gas configuration for Calcium would begin with
a)
[He]
b)
[Ar]
c)
[Ne]
d)
[Xe]
27.
The Lewis dot structure for Chlorine would have how many dots?
a)
2
b)
3
c)
7
d)
8
28.
An ionic compound is the result of
a)
2 nonmetals
b)
2 metals
c)
a metal and a nonmetal
29.
In a covalent bond, electrons are
a)
shared
b)
transferred
c)
erased
30.
What is the name for SO₂
a)
sulfur oxide
b)
disulfur oxide
c)
sulfur dioxide
d)
sulfur oxygen
31.
What is the formula for aluminum oxide?
a)
AlO
b)
Al2O3
c)
Al3O2
d)
Al3O
32.
Balance the following equation ___ H2 + ___ O2 → ____H2O
a)
2, 1, 2
b)
1, 2, 1
c)
2, 2, 2
d)
2, 3, 6
33.
According to the Law of Conservation of Mass, if an experiment starts with 10 grams of sodium and 15 grams chlorine, the product will be ______grams of sodium chloride.
a)
10
b)
15
c)
25
d)
5
34.
What type of reaction is pictured?
a)
synthesis
b)
depocomposition
c)
combustion
d)
single replacement
35.
A mole is the SI unit for
a)
the amount of a substance
b)
mass
c)
time
d)
volume
36.
A molecular formula is always the most simplified version of the formula.
a)
True
b)
False
37.
How many atoms are in 2 moles of water?
a)

1.204 x 10^24

b)
6.0 x 10^23
c)
0.3342
d)
0.053
38.
What percent of Na is in NaCl?
a)
39%
b)
50%
c)
61%
d)
23%
39.
Covalent bonds
a)
are between nonmentals that share electrons
b)
are between nonmentals that transfer electrons
c)
are between metals that share electrons
d)
are between metals that transfer electrons
40.
Which of the following is a compound?
a)
Al
b)
H2O
c)
H2
d)
salt and pepper
41.

Matter is anything that.....

a)

Has mass and takes up space

b)

Has mass and is visible

c)

Takes up space and has energy

d)

Has energy and is visible

42.

What particle view below is a mixture?

a)

b)

c)

d)

43.

What is an example of a chemical change?

a)

Tearing paper

b)

Dissolving salt in water

c)

Melting ice

d)

Burning wood

44.

The atom with the largest atomic radius in Group 8A is -

a)

Ar

b)

He

c)

Kr

d)

Rn

45.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

46.

Of the halogens (group 7A), which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

47.

How many valence electrons does Carbon have?

a)

4

b)

5

c)

6

d)

8

48.

What group is highlighted here on the periodic table (D-block elements)?

a)

Non-metals

b)

Metalloids

c)

Rare Earth Metals

d)

Transition Metals

49.
The image shows the periodic grid for POTASSIUM. How many PROTONS are found in a potassium atom?
a)
19
b)
39
c)
20
d)
Impossible to tell
50.
A(n) ____________________ is a pure substance made of a single type of atom and cannot be broken down.
a)
Element
b)
Compound
c)
Molecule
d)
Mixture
51.
What does the ATOMIC MASS tell us about an atom?
a)
Protons + Neutrons
b)
Protons + Electrons
c)
Neutrons + Electrons
52.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
53.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
54.

How many electrons can fit on the 1st energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

55.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
56.

___________ simplify the Bohr Model by showing only the outer valence electrons used for bonding.

a)

Lewis Dot Diagrams

b)

Bohr Models

c)

Electron Clouds

d)

Periodic Tables

57.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
58.

Which element would be in group 2?

a)

V

b)

W

c)

X

d)

Y

e)

Z

59.

What is this element? Use a periodic table!

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

60.

Which characteristic of a substance is considered a chemical property?

a)

its boiling point

b)

its reactivity

c)

its density

d)

its conductivity

61.

Which laboratory activity involves a chemical change?

a)

boiling saltwater for several minutes until only solid salt remains

b)

extracting iron filings from a sand mixture using a magnet

c)

leaving a copper penny in vinegar until it turns green

d)

crushing a rock with a hammer to extract mineral deposits

62.

NaBr

a)

Bromide sodide

b)

Sodium bromide

c)

Sodium bromate

d)

Sodium bromite

63.
Name this compound:
Li2SO3
a)
Lithium sulfate
b)
Lithium sulfite
c)
Lithite sulfide
d)
Sulfur lithite
64.
What is the formula for calcium oxide? 
a)
Ca2O2
b)
Ca2O
c)
CaO
d)
CaO2
65.
How many grams is 1.2 moles of Neon?
a)
0.05 grams
b)
16.6 grams
c)
21.2 grams
d)
24 grams
66.
Convert 28.0 grams of O2 to moles.
a)
1.14 moles
b)
1.75 moles
c)
0.571 moles
d)
0.875 moles
67.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

68.

Find the percent composition of CaCl2?

a)

Ca: 36.11%; Cl: 63.88%

b)

Ca: 53.12%; Cl: 100%

c)

Ca: 36.11%; Cl: 83.56%

d)

Ca: 46.11%; Cl: 63.88%

69.

JJ Thomson's experiment that he used to discover electrons

a)

gold foil experiment

b)

cathode ray experiment

c)

neither of these is correct

70.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
71.
Fe +2  and  SO4 -2
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
72.

Valence electrons are found

a)

in the innermost energy level of an atom

b)

in the middle energy levels of an atom

c)

in the outermost energy levels of an atom

73.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

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