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WorksheetsUnit 1 Exam Review_2022
Total questions: 47
Worksheet time: 38mins
Name
Class
Date
1.
How many protons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
10
c)
2
d)
18
2.
Which particle contributes the negative charge to the atom?
a)
proton
b)
electron
c)
neutron
d)
nucleus
3.
If two atoms possess the same number of protons, but contain a different number of neutrons then the two atoms are considered:
a)
Ions
b)
Isotopes
c)
Positive
d)
Negative
4.
What is true about metals on the periodic table?
a)
They are more numerous than other elements
b)
They are mostly on the left side of the table
c)
They are to the left of the zigzag(stairstep) line that starts with Boron
d)
All of the above
5.
Calculate the avg. atomic mass of chromium:
Cr-50 (mass of 49.946 amu & 4.35% abundance)
Cr-52 (mass of 51.941 amu & 83.79% abundance)
Cr-53 (mass of 52.941 amu & 9.5% abundance)
Cr-54 (mass of 53.939 amu & 2.36% abundance)
Choose the most correct answer.
Cr-50 (mass of 49.946 amu & 4.35% abundance)
Cr-52 (mass of 51.941 amu & 83.79% abundance)
Cr-53 (mass of 52.941 amu & 9.5% abundance)
Cr-54 (mass of 53.939 amu & 2.36% abundance)
Choose the most correct answer.
a)
52.25 amu
b)
52.19 amu
c)
52 amu
d)
51.996 amu
6.
Calculate the avg. atomic mass of Boron:
B-10 (mass of 10.013 amu & 19.8% abundance)
B-11 (mass of 11.009 amu & 80.2% abundance)
Choose the most correct answer.
B-10 (mass of 10.013 amu & 19.8% abundance)
B-11 (mass of 11.009 amu & 80.2% abundance)
Choose the most correct answer.
a)
10.812 amu
b)
10.511 amu
c)
10.5 amu
d)
10 amu
7.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
8.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
9.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
10.
Name this formula:
KNO3
a)
Potassium Nitrogen Oxide
b)
Potassium Nitride
c)
Potassium Nitrate
d)
Potassium (I) Nitrite
11.
What is the name of the compound SO2
a)
Monosulfate oxide
b)
Sulfur Dioxide
c)
Monosulfur dioxide
12.
Name the compound CuO
a)
copper (II) oxide
b)
copper oxide
c)
copper (I) oxide
d)
carbon uranium oxide
13.
The chemical formula of lead (IV) nitrate is
a)
PbN₄
b)
PbNO₃₄
c)
Pb(NO₃)₄
d)
Pb₃NO₄
14.
Fe+3 combines with S-2 to form
a)
Fe+4(S)=3
b)
Fe2S4
c)
Fe2S3
d)
Fe3S2
15.
What formula results when Fe+3 and CO3-2 ions bond?
a)
FeCO3
b)
Fe2CO3
c)
Fe2(CO3)3
d)
Fe3(CO3)2
16.
Identify the equipment shown here:
a)
test tube wire
b)
iron ring
c)
utility clamp
d)
test tube holder
17.
Identify the equipment shown here:
a)
beaker
b)
Erlenmeyer flask
c)
Florence flask
d)
volumetric flask
18.
How many sig figs are there?
0.000008
0.000008
a)
1
b)
2
c)
6
d)
7
19.
How many sig figs are there?
0.00400
0.00400
a)
1
b)
3
c)
5
d)
6
20.
How many significant figures will be in the answer to the following question:
7.62 x 6.98 x 3.2645
7.62 x 6.98 x 3.2645
a)
1
b)
2
c)
3
d)
4
21.
Calculate 5.50 cm + 5.50 cm and give your answer with the appropriate number of significant figures.
a)
11 cm
b)
11.0 cm
c)
11.00 cm
d)
11.000 cm
22.
Veal finds a gold colored rock in a river. It has a mass of 9.65 grams and a volume of 0.5 cm3. What is the density of the rock?
a)
10.15 g/cm3
b)
19.3 g/cm3
c)
9.15 g/cm3
d)
4.825 g/cm3
23.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
24.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
25.
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)
26.
What would you expect to see in a container labeled NaCl (aq)
a)
Solid salt granules
b)
Clear salt solution
c)
Water
d)
Liquefied salt
27.
What can be said about matter that is considered very dense?
a)
The particles are spread out within the volume of the matter
b)
The matter is very heavy
c)
The particles are closely packed together in a small volume
d)
The matter is light for it's relative size
28.
Which experimental evidence supports a model of the atom that consists of electrons distributed in a "pudding" of positive charge?
a)
Neutrons have similar masses to protons
b)
Electrons can be removed from materials
c)
Atoms form compounds
d)
Copper emits a green light in a flame test
29.
Use the data pictured to determine the color of the flame test when run with Lithium sulfate, Li2SO4
a)
Red
b)
Yellow-orange
c)
Orange
d)
Pink
30.
What is the correct reading for the volume of water in this graduated cylinder
a)
16 mL
b)
17 mL
c)
18 mL
d)
19 mL
31.
Which of the following statements is true about two blocks of gold that are different shapes but same mass?
a)
They have the same volume, but different densities
b)
They have different volumes, but same density
c)
They have different volumes and different densities
d)
They have the same volume and the same density
32.
Which of the following is an extensive property?
a)
hardness
b)
melting point
c)
density
d)
mass
33.
The chemical formula for the compound copper oxide is Cu2O. What is most likely to be true about the properties of copper oxide in relation to the properties of copper and oxygen?
a)
All three substances have similar properties
b)
Copper oxide has properties very similar to those of copper
c)
Copper oxide has properties very similar to those of oxygen
d)
All three substances have different properties
34.
What does the symbol (s) stand for?
a)
solid
b)
solution
c)
aqueous
d)
gas
35.
Most of the elements in the periodic table are...
a)
solid metals
b)
liquid metals
c)
gaseous nonmetals
d)
radioactive
36.
What group is the least reactive group of elements on the periodic table?
a)
alkali metals
b)
halogens
c)
noble gases
d)
transition metals
37.
The element gallium has two stable isotopes. 60% are gallium-69 and the remaining 40% are gallium-71. What is the average atomic mass of gallium?
a)
69.6
b)
70.2
c)
69.8
d)
70.4
38.
Which of the following is true in regards to isotopes of naturally occurring elements?
a)
The majority of radioactive isotopes are elements with atomic numbers less than 80
b)
The mass number of an isotope is almost always more than twice the atomic number
c)
Most atoms have only one stable isotope
d)
A few elements have isotopes with different atomic numbers and different mass numbers
39.
Which of the following descriptions correctly labels the pictured diagrams?
a)
a fluorine atom and a fluoride ion with a charge of -1
b)
a fluorine atom and a fluoride ion with a charge of +1
c)
a fluorine atom and a neon atom
d)
a neon ion with a charge of +1 and a neon atom
40.
The rule of zero charge states that...
a)
An atom that gains an electron must also gain a proton to remain electrically neutral
b)
an ionic compound contains two or more elements that have no charge
c)
the charges on metal cations and nonmetal anions in an ionic compound ad up to zero
d)
atoms gain neutrons when forming ionic compounds
41.
What is the metal to nonmetal ratio of ionic compounds formed from the two groups highlighted on the periodic table pictured?
a)
1:1
b)
2:1
c)
1:2
d)
2:7
42.
What conclusion can you draw from studying the diagram pictured?
a)
The outermost shell of every atom has eight electrons or fewer
b)
All of the subshells within a shell must be filled before any electrons can fill in the next shell
c)
With the exception of helium, the electron configuration for a noble gas in the nth period always ends with ns2np6
d)
The order in which subshells fill within a shell is s, p, f, and finally d
43.
What is the mass of 5.1 mL of mercury. The density of mercury is 13.6 g/mL
a)
69.4 g
b)
0.375
c)
2.67
44.
For Fluorine, what type of element is it, what is the phase at room temperature, and what group is it in?
a)
nonmetal, solid, halogen
b)
nonmetal, gas, halogen
c)
metal, solid, noble gas
d)
metalloid, liquid, alkali earth metal
45.
How many protons, neutrons, electrons, core electrons, valence electrons does fluorine have?
a)
9, 19, 9, 8, 1
b)
9, 10, 9, 2, 7
c)
9, 19, 9, 2, 7
d)
9, 9, 10, 8, 1
46.
How many valence electrons does sulfur (atomic number 16) have?
a)
16
b)
8
c)
6
d)
2
47.
What charge does the sulfide anion have?
a)
0
b)
-1
c)
-2
d)
+1
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