Worksheets***Gen Chem Midterm ***
Total questions: 100
Worksheet time: 5hrs 41mins
Name
Class
Date
1.
What is chemistry?
a)
The study of matter and the changes matter undergoes
b)
The study of energy and the movement and flow of energy between systems
c)
The study of how living things interact with the world and with each other
d)
The study of earth systems from begining to end
2.
What is matter?
a)
Items that take up space and you can see them
b)
Items that take up space and have mass
c)
Items that have mass and you can measure them
d)
Items that have mass and you can see them
3.
A ____________ is made up of one type of matter and cannot be separated by physical means.
a)
Pure Substance
b)
Mixture
c)
Heterogeneous Mixture
d)
Compound
4.
What does the particle diagram represents
a)
Pure Substance
b)
Homogenous Mixture
c)
Heterogeneous Mixture
d)
Compound
5.
_________ does not depend on the quantity (amount) of matter.
a)
Extensive Property
b)
Mixture
c)
Intensive Property
d)
Compound
6.
______________ A mixture that is the same throughout.
a)
Heterogeneous mixture
b)
Homogeneous mixture
c)
Element
d)
Compound
7.
____________ Two or more elements that are chemically bonded together.
a)
Heterogeneous mixture
b)
Homogeneous mixture
c)
Element
d)
Compound
8.
Salt Water is an example of a _______________.
a)
Heterogeneous mixture
b)
Homogeneous mixture
c)
Element
d)
Compound
9.
_____________ A change in appearance that does not change the chemical composition.
a)
Chemical Change
b)
Physical Change
c)
Chemical Property
d)
Physical Property
10.
Spoiled milk is an example of a _______________.
a)
Chemical Change
b)
Physical Change
c)
Chemical Property
d)
Physical Property
11.
Ice melting is an example of a _________________.
a)
Chemical Change
b)
Physical Change
c)
Chemical Property
d)
Physical Property
12.
The density of water is an example of a(n)
a)
Extensive Property
b)
Intensive Property
c)
Chemical Property
d)
Matter
13.
Accuracy is defined as ________ while Precision is _______
a)
Mass/Volume, How repeatable your results are
b)
How repeatable your results are, Mass/Volume
c)
How close your results are to the desired value, How close your results are to one another
d)
How close your results are to one another, How close your results are to the desired value
14.
If I measure a metal solid for mass and my measurements are 3.2 g, 4.3 g, 1.9 g and the true value of my metal's mass is 2.7g. My data is...
a)
Accurate
b)
Precise
c)
Both
d)
Neither
15.
Who discovered atoms exist?
a)
Democritus
b)
Dalton
c)
Johnson
d)
Rutherford
16.
Which solution is more dense?
a)
Blue
b)
Red
c)
Yellowish
d)
Clear
17.
Which subatomic particles tells you what element you have? Select all that apply
a)
Electrons
b)
Protons
c)
Neutrons
18.
Which subatomic particles make up an atom’s mass? Select all that apply
a)
Electrons
b)
Protons
c)
Neutrons
d)
Ions
19.
Which phrase describes an atom?
a)
a negatively charged nucleus surrounded by positively charged electrons
b)
a positively charged nucleus surrounded by negatively charged protons
c)
a positively charged nucleus surrounded by negatively charged electrons
d)
a negatively charged nucleus surrounded by positively charged protons
20.
Atoms are made of mostly _______ ________.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Empty Space
21.
F- is an example of a ___________ because it has ____________ one electron.
a)
Cation; gained
b)
Cation ; lost
c)
Anion ; gained
d)
Anion ; Lost
22.
The nucleus of an atom of Fluorine-19 contains
a)
9 protons and 10 neutrons
b)
10 protons and 9 neutrons
c)
19 protons and 9 neutrons
d)
19 protons and 19 neutrons
23.
An isotope is an atom of the same element that contains a different number of _________.
a)
Electrons
b)
Neutrons
c)
Protons
d)
Electrons and Protons
24.
Is this accurate, precise, neither, or both?
a)
Accurate
b)
Precise
c)
Both
d)
Neither
25.
What is a valence electron?
a)
Any electron in the atom
b)
An electron in the outermost shell of an atom
c)
An electron on the inside shell closest to the nucleus
d)
An electron that moves
26.
The atomic number in this element is
a)
9.0
b)
4
c)
5
d)
9.0122
27.
The atomic mass in this element is
a)
78
b)
117
c)
195
d)
195.085
28.
What is an orbital?
a)
a principal energy level
b)
An area of high probability for finding an electron
c)
A circular path which electron travel around the nucleus
d)
An elliptical path which electrons travel
29.
Neon has ______ valence electrons
a)
2
b)
8
c)
13
d)
18
30.
Silicon has ______ valence electrons
a)
4
b)
5
c)
7
d)
8
31.
In Bohr’s atomic model of Hydrogen, electrons are found at fixed distances from the nucleus known as __________ ___________.
a)
valence electrons
b)
empty spaces
c)
quantized levels
d)
energy levels
32.
The modern periodic table is organized by increasing ________________.
a)
atomic mass
b)
atomic number
c)
number of valence electrons
d)
element name
33.
Which of the following is a diatomic molecule?
a)
Bromine
b)
Phosphorus
c)
Neon
d)
Carbon
34.
How many electrons does the calcium ion have?
a)
20
b)
22
c)
18
d)
19
35.
What element is this?
a)
Lithium
b)
Sodium
c)
Neon
d)
Magnesium
36.
What orbital is this?
a)
s
b)
p
c)
d
d)
f
37.
How many electrons can this orbital hold by itself?
a)
4
b)
2
c)
3
d)
6
38.
How many orientations of this orbital are there?
a)
1
b)
7
c)
3
d)
5
39.
Name this compound: SiF4
a)
Sulfur (IV) TetraFluoride
b)
Silicon (IV) Fluoride
c)
Monosilicon TetraFluoride
d)
Silicon TetraFluoride
40.
Name this compound: N2O3
a)
Nitrogen (II) Oxide
b)
Nitrogen Oxide
c)
DiNitrogen Trioxide
d)
Trinitrogen Dioxide
41.
Name this compound: CuO
a)
Copper Oxide
b)
Copper Monoxide
c)
Copper (I) Oxide
d)
Copper (II) Oxide
42.
Name this compound: NH4Cl
a)
Ammonium Chloride
b)
Ammonium (IV) Chloride
c)
Nitrogen Tetrahydrogen Chloride
d)
Nitrogen Hydrogen (IV) Chloride
43.
Name this compound: Mg(NO3)2
a)
Magnesium (II) Nitrate
b)
Magnesium Nitrate
c)
Magnesium DiNitrate
d)
Magnesium Nitrate (II)
44.
Write the formula: Dinitrogen pentoxide
a)
2N5O
b)
N2O5
c)
N(II)O(V)
d)
NNO5
45.
Write the formula: Iron (II) Hydroxide
a)
Fe(OH)
b)
Fe2(OH)
c)
Fe(OH)2
d)
FeH
46.
Write the formula: Magnesium phosphate
a)
MgP
b)
Mg3P2
c)
Mg2(PO4)3
d)
Mg3(PO4)2
47.
Nobel gases ....
a)
Have full octets and generally do not bond; not very reactive
b)
Have full octets and bond readily; very reactive
c)
Have full octets and give electrons to those who need; very reactive
d)
Do not generally have full outer shells
48.
What is the mass of the following atom?
a)
3
b)
6
c)
10
d)
7
49.
Rutherford's Gold Foil Experiment showed what?
a)
Atoms have a positively charged nucleus
b)
Electrons are located in the center
c)
Atoms have a neutral nucleus
d)
Electrons and Protons are evenly spaced out in an atom
50.
How many neutrons are in gold?
a)
79
b)
197
c)
100
d)
118
51.
What state of matter is this?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
52.
What state of matter has a uniform composition, does not compress, and does not change to fit the shape of it's container?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
53.
When a system gives off heat energy it is considered
a)
Exothermic
b)
Endothermic
c)
Hypothermic
d)
In Equilibrium
54.
Where do electrons "live"?
a)
In the nucleus
b)
With the protons
c)
In electron clouds orbiting the nucleus
d)
In between energy levels
55.
Which of the following is an isotope of Silicon?
a)
14 protons, 14 neutrons
b)
14 protons, 15 neutrons
c)
14 protons, 15 electrons
d)
14 protons, 14 electrons
56.
What is an ionic compound composed of?
a)
A Cation and an anion
b)
2 Cations
c)
2+ metals
d)
2+ nonmetals
57.
What is an molecular compound composed of?
a)
A Cation and an anion
b)
2 Cations
c)
2+ metals
d)
2+ nonmetals
58.
Which is an Ionic Compound?
a)
SO2
b)
Na2O
c)
CH4
d)
F2
59.
Ionic compounds have___________ boiling points while molecular compounds have _____________ boiling points
a)
low, high
b)
no, weak
c)
high, low
d)
weak, no
60.
Which is a chemical property?
a)
Boiling Point
b)
Grinding
c)
Tearing
d)
Dissolves in acid
61.
Which of the following is a property of metals?
a)
low heat exhange
b)
unmalleable
c)
fragile
d)
conducts electricity
62.
Which is a metalloid?
a)
Aluminum
b)
Indium
c)
Arsenic
d)
Lead
63.
Which element has a larger electronegativity
a)
Aluminum
b)
Lithium
c)
Fluorine
d)
Helium
64.
Group 6, Period 4
a)
No element there
b)
Cesium
c)
Chromium
d)
Halfnium
65.
Iron is
a)
A metalloid
b)
In period 3
c)
In group 8
d)
In the "p" block of the periodic table
66.
What is periodicity?
a)
When the PTE is arranged by increasing atomic number, periods have similar properties
b)
When the PTE is arranged by decreasing atomic number, periods have similar properties
c)
When the PTE is arranged by decreasing atomic number, groups have similar properties
d)
When the PTE is arranged by increasing atomic number, groups have similar properties
67.
What is an ion?
a)
an element with the same protons but different mass
b)
an element with different protons but same electrons and neutrons
c)
an element that gains or loses electrons, but has a constant number or protons and neutrons
d)
an element with different protons and neutrons but same number of electrons
68.
What is different about ions of transition metals?
a)
they have roman numerals
b)
they are negatives
c)
they are polyatomic elements
d)
they do not exist
69.
Cations are ________ than their original atom, while Anions are ________ than their original atom.
a)
larger; smaler
b)
smaller; larger
c)
more electronegative; less electronegative
d)
less electronegative'; more electronegative
70.
What is the relationship between frequency and wavelength?
a)
when frequency goes up, wavelength goes up
b)
when frequency goes up, wavelength goes down
c)
when frequency goes down, wavelength goes down
d)
there is no relationship!!!
71.
Which color takes more energy to produce?
a)
red
b)
yellow
c)
blue
d)
violet
72.
How does light get emitted?
a)
electrons jump up to other energy levels by gaining energy
b)
electrons move up and down and that movement causes light
c)
electrons naturally have energy they need to shed
d)
electrons fall down from an excited energy level by releasing energy
73.
Where are we most likely to find electrons in an atom, according to the cloud model?
a)
Far away from the nucleus
b)
Closer to the nucleus
c)
In specific patterns around the nucleus
d)
Inside the nucleus
74.
What element is this: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2
a)
Iron
b)
Titanium
c)
Germanium
d)
Zirconium
75.
How many periods are on the periodic table?
a)
9
b)
7
c)
5
d)
18
76.
What is the ion formed from the Nitrogen atom
a)
N3+
b)
N3-
c)
N2+
d)
N2-
77.
What is this? (SO4)2-
a)
Sulfide
b)
Sulfate
c)
Sulfite
d)
Sulfur Tetraoxide
78.
What graph does this represent
a)
Endothermic Reaction
b)
Exothermic Reaction
c)
Heating Curve
d)
Cooling Curve
79.
Where are the Halogens located?
a)
Group 1
b)
Group 2
c)
Below the main periodic table
d)
Group 17
80.
At what number does the solution change from a liquid to a gas, undergoing evaporation
a)
1
b)
2
c)
3
d)
4
e)
5
81.
How many sig figs are in 0.010470
82.
12.1 + 7.935
83.
2.33 x 1.0
84.
Turn 4,832 into scientific notation (a)
Choose from the below words
4.832 x 10^3
4.832 x 10^-3
48.32 x 10^-2
48.32 x 10^2
85.
6.02 x 10^23 / 1.22 x 10^20
86.
If I have a cube with measurements of 1.30 cm by 1.30 cm by 1.30 cm, and it was put on a weight boat that measured 30.0 g with the sample in it. The weight boat itself weighs 28.0 g. What is the density of the cube?
87.
Joshua uses his thermometer and finds the boiling point of ethyl alcohol to be 75oC. He looks in a reference book and finds that the actual boiling point of ethyl alcohol is 90oC. What is his percent error?
88.
How many mL are in 2.24 L
89.
If I have 10 pounds of Molybdenum how many grams of Molybdenum do I have?
90.
If I can make 2 gal/day of water by combining 2 hydrogens with 1 oxygen, how many L/seconds of water can I make?
91.
Violet light has a wavelength of 3.98 x 10^-12 m. What is the frequency?
92.
Green light has a frequency of 4.77 x 10^14 Hz. What is the wavelength?
93.
Calculate the energy of a photon of radiation with a wavelength of 8.8 x 10^-7 m
94.
Draw the Lewis structure for Dihydrogen Monoxide (Water)
95.
Draw the Lewis structure for Lithium
96.
Rubidium is a soft, silvery-white metal that has two common isotopes, 85-Rb and 87-Rb. If the abundance of 85-Rb is 72.2% and the abundance of 87-Rb is 27.8%, what is the average atomic mass of rubidium?
97.
Write the electron configuration for Chlorine
98.
How many joules of heat are required to raise the temperature of 550 g of water, with a specific heat of 4.184 J/goC from 12.0 oC to 18.0 oC?
99.
Convert 61 kcal into kJ.
100.
Who is, indisputably, the most important person in Vault 101, he who shelters us from the harshness of the atomic Wasteland, and to whom we owe everything we have, including our lives.
a)
The Overseer
b)
THE OVERSEER
c)
THE overseer
d)
the OVERSEER
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