WorksheetsChemistry Semester 1 Review
Total questions: 68
Worksheet time: 34mins
Name
Class
Date
1.
A pure substance whose atoms are of the same type is called:
a)
Mixture
b)
Element
c)
Compound
2.
How many liquids in the cylinder are less dense than water?
a)
3
b)
2
c)
5
3.
Object B displaces water. Initial water level in a graduated cylinder is 20mL, and when object B is placed in water, the final water level is 28 mL. If its density is 6g/ mL, what is its mass in grams?
a)
48 g
b)
168 g
c)
1.3 g
d)
120 g
4.
Write 0.00278 in scientific notation.
a)
2.78x 10^ 3
b)
2.78x 10^-4
c)
2.78x 10^-3
d)
2.78x 10^4
5.
Convert 1.76 x 10^ -3 into standard notation
a)
0.00176
b)
0.0176
c)
176000
d)
1760
6.
What is a property of both matter and energy?
a)
They both have weight
b)
They both take up space
c)
Both cannot be created nor destroyed
d)
They don't have any properties in common
7.
a)
A
b)
B
c)
C
d)
D
8.
a)
a
b)
b
c)
c
d)
d
9.
When you touch an object and it feels hot, is it giving you energy or taking energy from you?
a)
Giving you Energy
b)
Taking your Energy
10.
How much energy is absorbed to bring 250g of room temperature water (25 C) to boiling temperature (100 C), knowing the specific heat of water is 4.18 J/gC
(a)
11.
a)
A
b)
B
c)
C
d)
D
12.
The sun heating up the earth is an example of:
a)
convection
b)
conduction
c)
radiation
d)
all of the above
13.
Hot coffee is stirred with a spoon , the spoon gets too hot due to
a)
radiation
b)
convection
c)
conduction
14.
Near the ceiling of a room the air is warmer. The warm air rises because of
a)
radiation
b)
convection
c)
conduction
15.
What does Fire need to happen?
a)
oxygen
b)
heat source
c)
fuel
d)
all of the above
16.
How many milliliters (mL) is .000239 Kiloliters (kL)?
(a)
17.
Heat flows from hotter objects to colder objects until it reaches a state where heat is no longer flowing. What have the objects reached when heat is no longer flowing?
a)
stable equilibrium
b)
thermal equilibrium
c)
chemical equilibrium
d)
mechanical equilibrium
18.
This diagram shows two closed, insulated compartments, where no energy can escape. Both compartments contain water of equal volume but varying temperatures of 50°C and 25°C respectively. If the temperature of the water measuring 50°C decreased by 5°C, the temperature of the water measuring 25°C would
a)
remain the same.
b)
also decrease by approximately 5°C.
c)
increase by approximately 5°C.
d)
none of the above
19.
The table displays the temperature of substance A and substance B placed near each other, but not touching, in a room at 25°C. Temperature was taken at three time intervals. Which of the following statements best supports the data in the table?
a)
Both substances lost energy.
b)
Both substances gained energy.
c)
Energy was lost by substance A to the environment.
d)
Energy lost by substance A was transferred to substance B.
20.
You have four water samples at different temperatures. In which sample are the molecules vibrating at the fastest speed?
a)
water at 100°C
b)
water at 100°F
c)
water at 100K
21.
You have two charges as shown in the image: A (which is positively charged) and B (which is negatively charged). If you insert a positive charge C in the middle of A and B, how would A and B move?
a)
A and B would move toward C.
b)
A would move toward C, and B would move away from C.
c)
A and B would move away from C.
d)
A would move away from C, and B would move toward C.
22.
15 Joules is _______kJ
a)
15kJ
b)
.015kJ
c)
1.5kJ
d)
15000kJ
23.
A celebrity chef is looking for a metal-plated pan that she can heat to as high a temperature as possible for a given input of energy. Her different pan options are copper (385 J/kg C°), iron (462 J/kg C°), and aluminum (903J/kg C°). All of the pans have the same mass. Observe each metal’s specific heat capacity . Which metal pan should the chef choose because it undergoes the largest temperature change for a given input of energy?
a)
The chef should choose the copper pan.
b)
The chef should choose the iron pan.
c)
The chef should choose the aluminum pan.
d)
The chef can choose any of the three pans, because all three pans will undergo the same amount of temperature change.
24.
When a piece of aluminum is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
-50°C
b)
50°
c)
-150°
d)
150°
25.
If 200 grams of water is to be heated from 20.0° C to 100.0° C to make a cup of tea. How much heat was added to the water? (c = 4.18 J/g⁰C).
a)
6,600 J
b)
3,828 J
c)
66,000 J
d)
66,880 J
26.
The temperature of a container of oxygen gas is increased from 149 K to 298 K.
Which of the following statements is true?
a)
The average kinetic energy of the oxygen molecules in the container decreases.
b)
The average chemical potential energy of the oxygen molecules in the container increases.
c)
The average kinetic energy of the oxygen molecules in the container increases.
d)
The average chemical potential energy of the oxygen molecules in the container decreases.
27.
a)
A
b)
B
c)
C
d)
D
28.
The temperature of 100g of water changed from 20C to 30C. How much heat in joules did this sample absorb? The specific heat of water is 4.18 J/gC
(a)
29.
a)
A
b)
B
c)
C
d)
D
30.
Automotive technology students are studying the combustion reactions that occur within a car’s combustion chamber.The students are studying the process of how controlled gasoline explosions that take place within a car’s engine change the potential chemical energy into the kinetic mechanical energy that moves the car.
Which of the following statements is true about this reaction?
a)
This is an exothermic reaction because energy is absorbed.
b)
This is an endothermic reaction because energy is absorbed.
c)
This is an endothermic reaction because energy is released.
d)
This is an exothermic reaction because energy is released.
31.
Given the specific heat of the substances below, which substance would heat up the slowest if left out in the sun?
a)
Liquid Water
b)
Solid Water
c)
Lead
d)
Dry Air
32.
What causes hot water to rise?
a)
Heat causes molecules to spread out, making it less dense
b)
Heat causes molecules to compact, making them more dense
c)
Heat pushes the water up through conduction
d)
Heat causes air to rise, pushing the water with it
33.
An atom is electrically neutral because it has equal numbers of protons and electrons.
a)
True
b)
False
34.
Which of the following represents a pair of isotopes?
a)
Ca+2, Be+2
b)
O-16, O-17
c)
Fe +2, Fe +3
d)
N, O
35.
How many neutrons are there in Ra-226?
a)
88
b)
138
c)
226
d)
314
36.
How many neutrons does Potassium (K) have? Round to the nearest whole number.
(a)
37.
Silicon is the second most abundant element in Earth’s crust. It is used in the electronics industry to manufacture transistors, and in the construction industry to produce concrete and Portland cement. The following graph shows the relative abundances of the naturally occurring silicon isotopes. Calculate the average atomic mass of Silicon using the information in the pie chart.
a)
26.2 amu
b)
28.1 amu
c)
29.8 amu
d)
30.1 amu
38.
Horizontal rows in the periodic table are called
a)
Blocks
b)
Groups
c)
Atomic mass
d)
Periods
39.
Which gas has less than 8 electrons in the valence shell of its atom ?
a)
Xe
b)
He
c)
Rn
d)
Ar
40.
a)
A
b)
B
c)
C
d)
D
41.
What element has 15 protons, 16 neutrons and 18 electrons
a)
P3-
b)
P
c)
P3+
d)
S
e)
S2+
42.
How many valence electrons does Iodine have?
(a)
43.
This could be a dotted structure of
a)
B
b)
S
c)
C
d)
Ca
44.
How many valence electrons does Sulfur have?
a)
6
b)
1
c)
2
d)
3
e)
4
45.
For the reaction below, the Water (H2O) and Oxygen (O2) could be referred to as:
a)
Product
b)
Reactant
46.
What are the products of any Combustion reactions:
a)
Oxygen gas and fuel
b)
Oxygen gas and Carbon Dioxide gas
c)
Carbon Dioxide gas and water
47.
A chemistry graduate student combines 3.90 grams of potassium and 12.7 grams of iodine to form potassium iodide. According to the law of conservation of mass, how much potassium iodide should be formed if the reaction proceeds to completion?
a)
0.0 grams
b)
8.8 grams
c)
16.6 grams
d)
33.2 grams
48.
Scientists created energy diagrams to correspond to various chemical reactions. These energy diagrams represented the energy changes of various reactants and products as the reactions take place. These diagrams showed that endothermic reactions absorb energy from their surroundings while exothermic reactions released energy into their surroundings. The diagrams also showed the activation energies associated with various reactions. Observe the graph. Which of the following statements is correct?
a)
The energy of the reactants is lower than the energy of the products.
b)
The energy of the reactants is higher than the energy of the products.
c)
The energy of the reactants is equal to the energy of the products.
d)
There is no energy absorbed during this reaction.
49.
Two iron blocks of equal size and mass are kept in contact with each other as shown in the figure. The block on the left side has been heated to 100°C and placed in contact with the block on the right side which has been cooled to 0°C. At thermal equilibrium, what would the temperature of the block measure on the left and right side?
a)
0°C, 0°C
b)
100°C, 0°C
c)
50°C, 50°C
d)
75°C, 25°C
50.
A science teacher set up a fish tank in her classroom to bring science to life. While cleaning the fish tank, a small piece of a plant broke away from the stem and floated upward and in the opposite direction of the heater. Upon reaching the opposite end of the tank, the plant piece gradually sank. It then floated back to the heater, where it rose once again. This movement repeated until the plant piece was removed from the fish tank.As water cools it becomes more dense. As water reached the surface of the tank it became cooler and began to sink. As the water sank, it heated again and moved upward again. The plant cycled around the tank with the moving water. This cycling of cool and warm temperatures is an example of
a)
expansion
b)
conduction.
c)
convection
d)
radiation.
51.
What is the lowest possible energy level that an electron can occupy?
a)
Excited state
b)
Ground state
c)
Fundamental state
d)
Outermost state
52.
A chemistry graduate student is very skilled at analyzing atomic emission spectra. The print out of her spectrum is printed in black and white. Therefore she has to rely on comparing the widths and positions of spectral lines during analysis. Observe the various atomic emission spectra. Which of the elements shown makes up the unknown spectrum?
a)
Copper
b)
Hydrogen
c)
Helium
d)
Sodium
e)
Strontium
53.
Which form of electromagnetic radiation has the greatest frequency?
a)
visible light
b)
gamma ray
c)
microwave
d)
infrared
54.
Based on the periodic table, which other element is likely to share common properties with sodium (Na)?
a)
Ca
b)
Cs
c)
Mg
d)
Ne
55.
The table shows the number of each of the three subatomic particles for four atoms. Which atoms represent the same element (are isotopes)?
a)
1 and 2
b)
2 and 3
c)
1 and 3
d)
2 and 4
56.
Choose the correct sequence of subshells in order from lowest to highest energy level.
a)
1s < 2s < 3s
b)
1s < 2p < 2s
c)
1s <2s < 2p
d)
1s < 2s < 3s < 2p
57.
The electron configurations of two unknown atoms are shown. Based on the electron configuration of each atom, what is the number of valence electrons for each atom?
a)
Atom X = 1; Atom Y = 1
b)
Atom X = 10; Atom Y = 10
c)
Atom X = 11; Atom Y = 17
d)
Atom X = 1; Atom Y = 7
58.
What is the identity of the element with the following electron configuration?
(a)
59.
Because ___________have the highest energy of all electromagnetic radiation, they are the most damaging to human tissue.
a)
Radiowaves
b)
Gamma Rays
c)
UV
d)
Visible light
60.
Which of the following is a characteristic of the Group 4 elements?
a)
They have 4 protons.
b)
They have 4 neutrons.
c)
They have 4 electrons.
d)
They have 4 valence electrons.
61.
An atom of bromine has 35 electrons. These electrons are present in energy shells around the nucleus. What is the electron configuration of bromine?
a)
2, 8, 18, 1
b)
2, 8, 18, 7
c)
2, 8, 18, 35
d)
2, 8, 8, 17
62.
The figure is a 3-dimensional representation of an atomic orbital. Which orbital does it represent?
a)
an s-orbital
b)
a single p-orbital
c)
three d-orbitals
d)
three p-orbitals
63.
The figure shows a 3D model of the shapes of a particular element’s atomic orbitals. If all the orbitals shown in the 3D model are completely filled, how many electrons does this element have?
a)
4
b)
6
c)
10
d)
18
64.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
65.
Select the correct order of waves on the EMS
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
66.
Put the visible light colors in order from longest wavelength to shortest wavelength
a)
Violet, Indigo, Blue, Green, Orange, Yellow, Red
b)
Red, Yellow, Green, Orange, Violet, Blue, Indigo
c)
Red, Orange, Yellow, Green, Blue, Indigo, Violet
67.
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
68.
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
a)
Nitrogen-13
b)
Nitrogen-14
c)
Nitrogen-15
d)
Based on the information given, it cannot be determined
100 %
