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WorksheetsMidterm Review - S1 - Chem 1
Total questions: 62
Worksheet time: 1hrs 7mins
Name
Class
Date
1.
DIFFERENT kinds of atoms chemically combined to form a substance are
a)
Mixture
b)
Element
c)
Compound
d)
Substance
2.
This contains a variety elements and compounds that ARE NOT chemically combined.
a)
Water
b)
Mixture
3.
A homogeneous mixture has the same composition of particles throughout.
a)
True
b)
False
4.
Alex goes into the garden and digs up a shovel full of dirt. This is a _____________ mixture.
a)
Homogeneous
b)
Heterogenous
5.
The image shown is an example of a ________.
a)
solution
b)
mixture
c)
suspension
6.
A combination of particles of one or more substance that are distributed uniformly throughout another substance is a/an
a)
Mixture
b)
Substance
c)
Solution
7.
What is the volume of 150 grams of lead if it has a density of 11.3 g/cm3?
a)
13.3 g
b)
13.3 cm3
c)
.075 g
d)
1695 cm3
8.
The density of this material is 2 g/cm3.
There are 24 cm3 Find the total mass.
There are 24 cm3 Find the total mass.
a)
12 grams
b)
48 grams
c)
12 g/cm3
d)
48 g/cm3
9.
Frank has a paper clip. It has a mass of 9g and a volume of 3cm3. What is its density?
a)
3 g/cm3
b)
1/3 g/cm3
c)
27 g/cm3
d)
39 g/cm3
10.
Who was the first to propose that all things are made of atoms?
a)
John Dalton
b)
Democritus
c)
Joseph Thomson
d)
Earnest Rutherford
11.
Who proposed the atomic theory?
a)
Democritus
b)
John Dalton
c)
Joseph Thomson
d)
Earnest Rutherford
12.
Who determined the nucleus is in the center of the atom?
a)
John Dalton
b)
Joseph Thomson
c)
Democritus
d)
Earnest Rutherford
13.
Who discovered the electron?
a)
Democritus
b)
John Dalton
c)
Joseph Thomson
d)
Earnest Rutherford
14.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
15.
Name an extensive properties
a)
color
b)
mass
c)
luster
d)
odor
16.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
17.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
18.
How many protons are present in phosphorus-31
a)
15
b)
16
c)
31
d)
46
19.
Found in the nucleus of the atom
a)
electrons only
b)
protons only
c)
neutrons and protons
d)
neutrons and electrons
20.
What does the 6 represent above the C
a)
Symbol
b)
Name
c)
Mass Number
d)
Atomic Number
21.
Atomic mass - Atomic Number =
a)
protons
b)
neutrons
c)
electrons
d)
Average Mass
22.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
23.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
24.
Copper occurs naturally as Cu-63 and Cu-65. Which isotope is more abundant?
a)
Cu-63
b)
Cu-65
25.
Calculate the average atomic mass of element X when 34% of element X exists as X-272 and the remainder exists as X-274.
a)
185.64amu
b)
273.32amu
c)
272.68amu
d)
27.33amu
26.
Which Elements is a metalliod
a)
Gallium
b)
Calcium
c)
Aluminum
d)
Germanuim
27.
Which is an example of chemical change
a)
Breaking Glass
b)
Tearing clothes
c)
Baking Cookies
28.
What is the law of conservation of mass?
a)
The part of the universe being studied
b)
The rest of the universe that interacts with the system
c)
Mass is not created nor destroyed, only can be rearranged.
d)
A system that freely exchanges matter and energy
29.
Suppose a reaction were to happen in an open container in a lab. During the reaction, the scientist observes the chemicals bubble, and produce a gas. During the analysis the scientist notices that the reactants had a mass of 20 g when he started, and the product only had a mass of 18 g. Explain what happened.
a)
His chemical reaction defied the law of conservation of mass
b)
The product destroyed mass during the reaction
c)
The reactants created matter during the reaction
d)
The gas that was produced was not able to be measured since the container was open.
30.
10 g of a solid chemical reacts with a 10 g of a liquid chemical, the reaction bubbles and changes the color of the liquid. The colored liquid weighs 13 g, what can be concluded?
a)
The gas produced from the bubbles measured 5 g
b)
The bubbles were evidence of 7 g of matter being destroyed
c)
The gas produced measured 7 g
d)
The gas produced measured 13 g
31.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
32.
Which element belongs to this longhand electron configuration
1s2 2s2 2p6 3s2 3p6 4s2 3d7
1s2 2s2 2p6 3s2 3p6 4s2 3d7
a)
Calcium
b)
Cobalt
c)
Nickel
d)
Copper
33.
What is this element?
[Ne] 3s23p64s2
[Ne] 3s23p64s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
34.
What is the noble gas shorthand for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
35.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
36.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
37.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
38.
Calcium is most like which of the following?
a)
Barium
b)
Potassium
c)
Cesium
d)
Nitrogen
39.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
40.
Elements which are considered semiconductors are
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
41.
The atoms along the staircase are called
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
42.
Which of the following is not a property of metals?
a)
brittle
b)
malleable
c)
lustrous
d)
conductive
43.
Good conductor of heat
a)
Metal
b)
Nonmetal
44.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
45.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
46.
What is the name of the group that never reacts--ever ever they are stable with a full outermost ring!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
47.
Which pair of elements is MOST similar?
a)
Ca and F
b)
Li and H
c)
Na and Cl
d)
Ne and Ar
48.
Which has the greater EN:
Cl or Al?
Cl or Al?
a)
Cl
b)
Al
49.
Which has the greater EN:
N or C?
N or C?
a)
C
b)
N
50.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
51.
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)
52.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
53.
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
54.
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.
55.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
c)
liquid properties
d)
real properties
56.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
57.
Is hammering wood together to build a house a chemical or physical change?
a)
chemical
b)
physical
58.
A change in the size, shape, or state of matter.
a)
chemical change
b)
physical change
c)
chemical reaction
d)
electron change
59.
Kim puts an ice cube in a beaker and it melts. This is a good example of:
a)
a physical change.
b)
a chemical change.
c)
an experiment.
d)
an analysis.
60.
Water and alcohol are easily separated by distillation because of their
a)
different densities
b)
different boiling points
c)
different colours
d)
different melting points
61.
Water is an element
a)
true
b)
false
62.
What is the atomic mass of Neon?
a)
10
b)
20.18
c)
10.18
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