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HGHS 2021 chemistry final review Flashcards | StudBud
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HGHS 2021 chemistry final review
HGHS 2021 chemistry final review
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Subatomic Particle Quiz.
Flashcards
57 cards
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Practice quiz
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Questions
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Answers
1
Put this equation into word form. Rb + P → Rb3P
rubidium combined with potassium forms rubidium phosphide
rubidium and phosphorus react to form rubidium phosphide
rubidium and potassium react to form rubidium potasside
rubidium plus potassium forms rubidium potasside
2
Using the stock name method when naming a transition metal ion the charge is indicated by a _____.
Roman numeral following the name
Arabic number following the name
Prefix
Superscript after the name
3
Which of the following allows metals to be good conductors of electricity?
protons
electrons
cations
neutrons
4
What is the formula for this compound: nitrogen trihydride?
NH₃
NH
N₃H₃
N₃H
5
How many moles of hydrogen atoms are present in 1 mole of H₂ gas?
3
4
2
1
6
The best instrument to use to measure volume in the lab is a _____.
test tube
beaker
flask
graduated cylinder
7
What is the electron configuration for zirconium?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2
1s2 2s2 2p6 3s2 3p6 3d10 4p6 5s2 4d2
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2 4d2
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d2
8
Which of the following gives the correct charges for the subatomic particles?
The neutron is positive, proton is negative, and electron is neutral.
The neutron is positive, electron is negative, and proton is neutral.
The proton is positive, electron is negative, and neutron is neutral.
The proton is positive, neutron is negative, and electron is neutral.
9
What is the mole ratio of oxygen to carbon dioxide in the combustion reaction for propane? C3H8 + 5O₂ → 3CO₂ + 4H₂O
5:1
1:5
5:3
3:5
10
Which of the following make up ionic compounds?
non-metal cations and non-metal anions
metal cations and non-metal anions
non-metal cations and metal anions
metal cations and metal anions
11
A chemical change always includes _____.
a new substance forming
a change in color
a change of mass
a change in the state of matter
12
Elements form into compounds in what ways?
Unpredictable
In only one way
Predictable
In an infinite number of ways
13
What is the chemistry definition of a mole?
a unit used to measure an extremely large quantity of things
an animal that runs around and can barely see
a type of pesticide that clears out weeds
the name of a scientist who wanted to count atom
14
In the quantum mechanical model of the atom, the energy levels are broken up into these sublevels
s, p
s, p, d
1, 2, 3, 4
s, p, d, f
15
How are chemical formulas of binary ionic compounds generally written?
Roman numeral first, then anion, then cation
anion on the left, cation on the right
subscripts first, then ions
cation on the left, anion on the right
16
An atom of neon has ten protons and a mass number of eighteen. How many neutrons does it have?
8
18
1
10
17
How many significant digits are there in 5.00920?
5
6
3
4
18
Why did Dimitri Mendeleev leave open spaces on his periodic table?
to divide metals from nonmetals
for elements that were yet to be discovered
no one is sure
to make it easier to read
19
How many atoms or molecules are in a mole?
6.02 x 10
1
6.02 x 10²³
2
20
What mass of silver is produced from 100.0 g Cu? Cu + 2Ag(NO3) → 2Ag + Cu(NO3)2
526 g
100 g
200.4 g
339.5 g
21
Covalent bonds exist when combining atoms _____.
Give up or accept electrons
Share electrons
Transfer electrons
Transfer or share electrons
22
What is the charge of an ionic compound?
neutral
negative
they do not have a charge
positive
23
Which of the following cannot be broken down by a chemical change?
water (H2O)
glucose (C6H12O6)
baking soda (NaHCO3)
sodium (Na)
24
Which of the following diatomic molecules is joined by a double covalent bond?
He2
Cl2
N2
O2
25
How many moles are present in 450 grams of sodium phosphide, Na₃P?
99.9
4.5
450
44,995
26
A pure substance could be a(n) _____.
element and compound
compound only
element only
element, compound, or mixture
27
In the formula H₂SO₄, what is the 4 called?
a subscript
a superscript
an exponent
a coefficient
28
Using prefixes, name this molecule: H₂O
dihydrogen monoxygen
monohydrogen dioxide
dihydrogen monoxide
monohydrogen dioxygen
29
What formula is used to represent the compound sulfur hexafluoride?
S₂F₅
SF₆
SF₇
SF₅
30
Identify this reaction. NH₃+H₂SO₄→(NH₄)₂SO₄
Decomposition
Single displacement
Synthesis
Double displacement
31
When do the particles in a in a glass of water stop moving?
They stop when the water freezes.
They stop when the water becomes ice.
They never stop moving.
They stop when the water evaporates.
32
C6H12O6 + 6O2 → 6H2O + 6CO2 uses 1 g of both C6H12O6 and O2. What is the percent yield if 0.45g of H2O is produced?
100%
80%
0.558%
0.31%
33
A diatomic molecule has _____ atom(s)
2
4
3
1
34
The name of As₂S₅ is _____.
diarsenic pentasulfide
arsenicdi pentasulfide
diarsenic pentasodium
diastatine pentasulfide
35
What is the symbol for iron?
I
Ir
In
Fe
36
Which equation represents a balanced chemical equation?
P₄+O₂→2P₂O₃
K+Cl₂→2KCl
CF₄+2Br₂→CBr₄+2F₂
N₂+3F₂→NF₃
37
Which subatomic particle(s) determine the identity of an element?
neutrons
protons and electreons
electrons
protons
38
Which of the following is an example of a compound?
sodium chloride
carbon
Oxygen
gold
39
What happens when the correct amount of carbon is added to iron to make carbon steel?
It becomes more durable and stronger.
Carbon and iron do not mix.
It becomes soft enough to make jewelry.
It becomes brittle.
40
What are the two features that distinguish something as matter?
takes up space and can move
has mass and weight
has mass and takes up space
has mass and can move
41
How many particles are present in 10.0 moles of table salt?
3.01 x 10²³ particles
6.02 x 10²³ particles
6.02 x 10²² particles
6.02 x 10²⁴ particles
42
Which element has the symbol Sn?
sodium
antimony
tin
sulfur
43
Which of the following is the formula for hydrobromic acid?
H₃B
HBrO₃
HBrO₂
HBr
44
What is the electron geometry of the nitrogen (N₂) molecule?
tetrahedral
Bent
Linear
trigonal planar
45
If the empirical formula of a compound is CH₂, which of the following could be a possible molecular formula?
C₂H₄
C₂H₂
CH₄
CH
46
On a cold day, water droplets collect on the inside of a window. This is an example of ____.
condensation
evaporation
melting
sublimation
47
Determine the molar mass of lactose, C₁₂H₂₂O₁₁.
342 g/mol
29 g/mol
171 g/mol
45 g/mol
48
Which of the following is an example of a physical change?
wood burning
metal rusting
cooking an egg
water evaporating
49
How many moles of helium gas are present in 120 liters at STP?
5.00
10.5
5.4
6.5
50
What is the average atomic mass of chlorine?
18 amu
36 amu
35 amu
17 amu
51
Identify this reaction. HCl+NaOH→NaCl+H(OH)
Synthesis
Combustion
Double displacement
Single displacement
52
Most polyatomic ions will only contain _____.
metal atoms
non-metal atoms
metal and non-metal atoms
neutral atoms
53
How many moles are represented by 3.01 x 10²⁴ oxygen atoms?
10
5
2
250
54
C6H12O6 + 6O2 → 6H2O + 6CO2 Which reactant is the limiting reagent if there is 1 gram of both C6H12O6 and O2?
O2
CO2
H2O
C6H12O6
55
Which element on the periodic table has sixteen protons?
germanium
oxygen
sulfur
cadmium
56
Which electrons are involved in chemical reactions?
The electrons found in the innermost energy level
The electrons found in the outermost energy level
All electrons are involved in chemical reactions.
The electrons found near the middle of the energy level
57
How many atoms of sulfur are there in Al₂(SO₄)₃?
3
2
4
12
