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Chemistry Science District Assessment

Total questions: 100

Worksheet time: 4hrs 30mins

Name
Class
Date
1.

What is the correct name for the following compound? Li 2 S

a)

Dilithium monosulfide

b)

Lithium disulfide

c)

Sulfuric lithate

d)

Lithium sulfide

2.

What is the name of the compound NiSO 4?

a)

Nickel (II) sulfate

b)

Nickel (II) sulfite

c)

Nickel (II) sulfide

d)

Nickel (II) sulfuroxide

3.

What is the correct name for the following compound? Al(NO 3 ) 3

a)

Aluminum trinitrate

b)

Aluminum nitrate

c)

Aluminum dinitrate

d)

none of the above

4.

What is the average atomic mass of neon? Isotope Mass number (grams) Percent Abundance (%) Ne- 20 90.48 Ne- 21 10.27 Ne- 22 29.25

a)

10.50 amu

b)

20.19 amu

c)

21.00 amu

d)

18.77 amu

5.

Which of the following showed electrons in specific, fixed orbits?

a)

Rutherford Model

b)

Planck Model

c)

Bohr Model

d)

Quantum Model

6.

Which of the following equations is an exothermic reaction?

a)

H 2(g) + ½ O 2(g) → H 2 O (l) ΔH = -285.8 kJ

b)

HgO (s) → Hg (l) + ½ O 2(g) ΔH = +90.7 kJ

c)

4CO 2(g) +6H 2 O (l) →2C 2 H 6 (g) +7O 2(g) ΔH =+3120 kJ

d)

SO 2 (g) → S (s) + O 2 (g) ΔH = +296 kJ

7.

Some physical properties of elements in a group of the Periodic Table are described below. The elements described above belong to which group?

a)

Alkaline earth metals

b)

Noble gases

c)

Alkali metals

d)

Halogens

8.

Which family correctly represents the elements in Group 1 on the Periodic Table?

a)

Transition metals

b)

Alkali metals

c)

Lanthanide elements

d)

Actinide series

9.

Charles' law says that if a certain quantity of gas is held at constant pressure, then its volume is directly proportional to the absolute temperature. Which of the following does this law help explain? Select TWO correct answers.

a)

Some gases only react at high temperatures.

b)

A basketball outside will shrink some as the temperature goes down.

c)

A gas-filled balloon expands upon heating.

d)

Solids require high heat in order to change into gases.

e)

The pressure of a gas increases when volume increases.

10.

The volume of a gas is 50.0 mL at 20.0 K. What will be the new temperature if the gas is compressed to 10.0 mL under constant pressure?

a)

100 K

b)

10.0 K

c)

4.00 K

d)

5.00 K

11.

Which element in Period 2 has the greatest tendency to form a negative ion?

a)

lithium

b)

carbon

c)

neon

d)

fluorine

12.

The electron configuration of potassium is -

a)

1s 2 2s 2 2p 6 3s 2 3p 2 4s 1

b)

1s 2 2s 2 2p 10 3s 2 3p 2 3p 3

c)

1s 2 2s 2 3s 2 2p 6 3d 1

d)

1s 2 2s 2 2p 6 3s 2 3p 6 4s 1

13.

What is the formula for iron (III) oxide?

a)

FeO 3

b)

Fe 3 O

c)

Fe 2 O 3

d)

FeO

14.

The chemical formula for the ionic compound formed when the elements of Ca and N react is -

a)

CaN

b)

Ca 2 N 3

c)

Ca 3 N 2

d)

Ca 5 N 2

15.

What is the correct formula for sodium phosphate?

a)

Na 2 P 2 O 4

b)

Na 2 PO 3

c)

Na 2 P 3 O 4

d)

Na 3 PO 4

16.

Which of the following is the correct electron dot formula for magnesium chloride?

4 lines
17.

The data table below shows elements Xx, Yy, and Zz from the same group on the periodic table. What is the most likely atomic radius of element Yy?

a)

103 pm

b)

127 pm

c)

166 pm

d)

185 pm

18.

Conductivity in metal results from metal atoms having -

a)

high electronegativity

b)

high ionization energy

c)

highly mobile protons in the nucleus

d)

highly mobile electrons in the valence shell

19.

What is the shape of a molecule which has two shared pairs of electrons and no unshared pairs?

a)

tetrahedral

b)

bent

c)

trigonal planar

d)

linear

20.

Which of the following correctly matches a compound with its molecular geometry? Select TWO correct answers.

a)

Borane (BH 3): trigonal planar

b)

water (H 2 O): linear

c)

carbon dioxide (CO 2): tetrahedral

d)

methane (CH 4): tetrahedral

e)

carbon tetrachloride (CCl 4): linear

21.

The Lewis dot structure determines the molecular geometry based on bonded and unbonded electrons. What is the expected molecular geometry for CO 2 ?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal planar

22.

Visible light has a higher frequency than radio waves on the electromagnetic spectrum. How does the wavelength of visible light compare to radio waves?

a)

Visible light has a longer wavelength than radio waves.

b)

Visible light has a shorter wavelength than radio waves.

c)

Visible light has the same wavelength as radio waves.

d)

Visible light does not have a wavelength while radio waves do have a wavelength.

23.

Energy is measured in........

a)

Wavelength

b)

Meters

c)

Joules

d)

Frequency

24.

On a wave, the distance between crest to crest is called?

a)

amplitude

b)

wavelength

c)

frequency

d)

trough

25.

Which color in the visible spectrum of light has the longest wavelength?

a)

Indigo

b)

Red

c)

Blue

d)

Violet

26.

Gamma rays can cause damage to living tissues because...

a)

They have medium wavelengths that can interfere with cell replication.

b)

They have very long wavelengths that can interfere with cell replication.

c)

They have very short wavelengths that can interfere with cell replication.

d)

None of these

27.

What does "h" stand for?

a)

Speed of Light

b)

Plank's Constant

c)

Speed of Sound

d)

Constant Energy

28.

The number of cycles in a given amount of time is ...

a)

longitudinal wave

b)

frequency

c)

diffraction

d)

reflection

29.

What does energy have to do with wavelength and frequency?

a)

The higher the frequency the less energy the wave has.

b)

The lower the frequency the more energy the wave has.

c)

The shorter the wavelength the more energy the wave has.

d)

The longer the wavelength the more energy the wave has.

30.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
31.
Which has the greater EN: 
N or C?
a)
C
b)
N
32.
Which has the greater EN: 
H or F?
a)
H
b)
F
33.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
34.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
35.
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)
36.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
37.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
38.
As you move down 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 nuetrons
39.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
40.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
41.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
42.
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
43.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
44.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
45.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
46.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

47.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
48.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
49.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
50.

What is the name of this group?

a)

alkali metals

b)

alkaline earth metals

c)

transition metals

d)

halogens

e)

noble gases

51.

What is the name of this group?

a)

alkali metals

b)

alkaline earth metals

c)

transition metals

d)

halogens

e)

noble gases

52.

How many valence electrons does this group have?

a)

1

b)

2

c)

7

d)

8

53.

What charge do ions of this group have?

a)

+1

b)

+2

c)

-2

d)

-1

e)

0

54.

What is the charge of this group?

a)

+1

b)

+2

c)

-2

d)

-1

e)

0

55.

Which element has an atomic radius that is LARGER than sodium?

a)

Lithium (Li)

b)

Hydrogen (H)

c)

Magnesium (Mg)

d)

Potassium (K)

56.

Which element has an atomic radius that is SMALLER than boron?

a)

beryllium (Be)

b)

aluminum (Al)

c)

carbon (C)

d)

Gallium (Ga)

57.

When oxygen becomes an ion, does it get larger or smaller?

a)

larger

b)

smaller

c)

depends on which isotope of oxygen it is

d)

oxygen forms several ions so it's impossible to tell

58.

The ionic radius of metals is

a)

larger than the metal atom

b)

smaller than the metal atom

c)

the same size as the metal atom

d)

trick question, metals don't form ions

59.

The ionic radius of noble gases is

a)

larger than the atom

b)

smaller than the atom

c)

the same size as the atom

d)

trick question, noble gases don't form ions

60.

Based on the trends we learned, which has the highest electronegativity?

a)

phosphorus (P)

b)

sulfur (S)

c)

arsenic (As)

d)

selenium (Se)

61.

Based on the trends we learned, which has the lowest ionization energy?

a)

phosphorus (P)

b)

sulfur (S)

c)

arsenic (As)

d)

selenium (Se)

62.

Which element has only two electron shells ?

a)

Helium (He)

b)

Neon (Ne)

c)

Argon (Ar)

d)

Krypton (Kr)

63.

Which element has two valence electrons?

a)

Helium (He)

b)

Neon (Ne)

c)

Argon (Ar)

d)

Krypton (Kr)

64.

You discover a new element, Osbornium. It has an atomic number of 434 and an atomic mass of 2451.434. How many protons does it have?

a)

434

b)

2451

c)

2451.434

d)

2017

65.

You discover a new element, Osbornium. It has an atomic number of 434 and an atomic mass of 2451.434. How many neutrons does it have?

a)

434

b)

2451

c)

2451.434

d)

2017

66.

Which is the most electronegative element of the ones given?

a)

lithium (3)

b)

cesium (55)

c)

oxygen (8)

d)

oganesson (118)

67.

Of the elements given, which one has the highest ionization energy?

a)

lithium (3)

b)

cesium (55)

c)

oxygen (8)

d)

oganesson (118)

68.

Of the elements given, which one is the smallest?

a)

lithium (3)

b)

cesium (55)

c)

oxygen (8)

d)

oganesson (118)

69.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
70.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
71.
What is the atomic number for an element with three protons?
a)
2
b)
1
c)
3
d)
6
72.

The atomic mass of an element is the ___.

a)

average of the mass number and the atomic number for the element

b)

weighted average of the masses of the isotopes of the element

c)

total mass of the isotopes of the element

d)

total number of subatomic particles in the nucleus

73.

Calculate the average atomic mass of the element iron (Fe) using the following data:

[Isotope / % abundance]

[Iron 54 / 6% ] [Iron 56 / 92% ] [ Iron 57 / 2% ]

a)

53.7 amu

b)

54.9 amu

c)

5592.0 amu

d)

55.9 amu

74.
An isotope has three forms.  30% have a mass of 4 amu, 20% have a mass of 5 amu and 50% have a mass of 3 amu.  Average atomic mass will be closest to
a)
2 amu
b)
3 amu
c)
4 amu
d)
5 amu
75.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
76.
For a given element, the atomic number indicates the number of _____
a)
protons in the nucleus
b)
neutron in the nucleus
c)
electrons in the atom
d)
nucleons in the atom
77.
If an atom contains exactly three protons, then it's an atom of _____
a)
lithium
b)
gold
c)
nitrogen
d)
carbon
78.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
79.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
80.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
81.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
82.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
83.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
84.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
85.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

86.

Name the type of enthalpy for the following reaction:

Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1

a)

Standard enthalpy of neutralisation, ΔHneuto

b)

Standard enthalpy of solution, ΔHsolno

c)

Standard enthalpy of hydration, ΔHhydo

d)

lattice energy, ΔHlatticeo

87.

What type of reaction is shown in the graph?

a)

endothermic reaction

b)

exothermic reaction

88.

C+ O2 --> CO2 + 60kJ

what is the ΔH for the reaction?

a)

+60

b)

-60

c)

there is no way to know

89.
Endothermic reactions feel
a)
warm
b)
cold
90.
(Hess's Law)Calculate the ∆H for the following reaction: 2H2O2 →  2H2O  + 1 O2 
You are given these two equations:
2H2  +  O2 → 2H2O            ∆H  =  -572 kJ
 H2  +  O2  →  H2O2            ∆H  =  -188 kJ 
a)
∆H  =  -948 kJ 
b)
∆H  =  -196 kJ 
c)
∆H  =  -384 kJ 
d)
∆H  =  -188 kJ 
91.

A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?

a)

0.777 atm

b)

1.65 atm

c)

1.28 atm

d)

0.61 atm

92.
Three gases, Ar, N2 and H2 are mixed in a sealed container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
93.

Which of the following is a TRUE statement based on the Kinetic Molecular Theory?

a)
Gases do not move in straight line
b)
Most of the volume of gas is empty space
c)
Gas particles are not in constant random motion
d)
Gas particles attract each other
94.

How many moles of oxygen must be placed in a 3.00 liter container in order to exert a pressure of 2.00 atmospheres at 25.0 °C?

a)

146.8 moles

b)

0.245 moles

c)

21778 moles

d)

4.08 moles

95.

When 0.250 moles of a gas is placed in a container at 25.0 °C, it exerts a pressure of 700.0 mm Hg. What is the volume of the container?

a)

0.557 Liters

b)

6.64 Liters

c)

8.74 Liters

d)

0.0087 Liters

96.
Which law?
a)
Charles 
b)
Boyle
c)
Hunsecker
d)
Newton
97.

Which of the following statements about the particles of a gas is true?

a)
Gases can be compressed because their particles are smaller than those of liquids or solids.
b)
Gases can be compressed because there is plenty of space between their particles.
c)
Gases can be compressed because they have low boiling points.
d)
Gases can be compressed because their particles are more elastic than those of liquids or solids.
98.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

99.

A sample of helium gas occupies 2.65 L at 1.20 atm. What pressure would this sample of gas exert in a 1.50 L container at a constant temperature?

This is Open-Ended Question A. Show your work on the answer sheet in the appropriate box on the paper, then type the answer in the box here. Do not include anything other than numbers and decimal points in this box.

(a)  

100.

A sample of oxygen gas (O2) has a volume of 7.51 L at a temperature of 19.0°C and a pressure of 1.38 atm. Calculate the number of moles of O2 present in this gas sample. (Answer to 3 decimal places)

This is Open-Ended Question C. Show your work on the answer sheet in the appropriate box on the paper, then type the answer in the box here. Do not include anything other than numbers and decimal points in this box.

(a)  

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