Why is Zirconium larger than Titanium?

Greater number of electron shells

Why is Chlorine more likely to gain electrons than Sulfur ?

The valence shell is closer to full

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Spring Final Exam Review

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Unit 6: Aqueous Reactions Unit 7: Nuclear Chemistry Unit 8: Periodic Table Trends Unit 9: Chemical Bonding Unit 10: Liquids and Solids Unit 11: Gases

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Questions 109

Answers

1
Why is Zirconium larger than Titanium?
Larger effective nuclear charge (Zeff)
The valence shell is closer to empty
Greater number of electron shells
The valence shell is closer to full
2
Which IMF would hold this substance together as a liquid?
Dipole-dipole
Ion-dipole
London Dispersion
Hydrogen bonding
3
What must be considered to find the polarity of covalent bonds?
Electronegativity
Electron Affinity
Ionization Energy
Dipole moment
4
Which type of crystals possess non-specific bonds allowing the materials to be deformed?
Mettalic
Ionic
Molecular
Covalent
5
Which pH would indicate a neutral solution?
6
5
8
7
6
What would be the precipitate if the following solutions were mixed? AgClO₃ & BaBr₂
AgCl
AgBr
Ba(ClO3)2
BrClO3
7
Which IMF would hold this substance together as a liquid?
Hydrogen bonding
Ion-dipole
London Dispersion
Dipole-dipole
8
Which compound has an incomplete octet?
SF6
BH3
CF4
OF2
9
Which element is most likely to gain an electron?
Calcium
Bromine
Krypton
Silver
10
Which gas law explains how chemical reactions produce work?
Boyles
Avogadro
Charles
Ideal gas law
11
How many sigma bonds are found in HCN?
0
2
1
3
12
Which of the following is not a property of nuclear fusion?
Requires incredibly hot temperatures
Radioactive decay
Used in particle accelerators
Smaller nuclei combining into larger ones
13
If each gas is found at the same temperature, which will have the lowest average velocity?
Equal
Ne
He
Kr
14
Which property is the resistance of fluid flow?
Surface tension
Viscocity
Adhesion
Capillary action
15
Which gas law relates volume and moles?
Ideal gas law
Charles
Boyles
Avogadro
16
Which phase transfer goes from solid directly to the gas phase?
vaporization
evaporation
sublimation
deposition
17
What type of molecules do not dissolve easily into water?
Non-polar
Polar
Neutral
Charged
18
Which is NOT something that could be found at a crystal’s lattice point?
Ions
Molecules
Covalent bonds
Atoms
19
Which phase transfer goes from a gas directly to the solid phase?
deposition
sublimation
evaporation
vaporization
20
What is the most electronegative element?
O
Ne
F
Cl
21
What is the second most abundant gas in air?
Helium
Argon
Oxygen
Nitrogen
22
What is the oxidation number of carbon in CF₄?
-4
+4
+2
+3
23
How can paperclips float on water?
Surface tension
Capillary action
Meisner effect
Leidenfrost effect
24
What is specifically being exchanged in a redox reaction?
Ions
Protons
Electrons
Neutrons
25
How many bonds will Nitrogen form when it has a -1 charge on the atom?
1
4
3
2
26
Who sorted the periodic table by mass & properties as well as left spaces for new elements?
Dmitri Mendeleev
Johann Dobereiner
Henry Moseley
John Newlands
27
Which of the following would NOT effect the gas volume?
Increasing moles
Increasing pressure
Increasing molar mass
Increasing temperature
28
What is specifically being exchanged in an acid - base reaction?
Protons
Electrons
Neutrons
Ions
29
Which elements would form brittle solids with low melting points?
Metalloid
Non-metalloid
Metals
Non-metals
30
How many non-bonding pairs of electrons are found in the Lewis structure of ammonia (NH₃)?
0
2
3
1
31
How many bonds will oxygen form when it has a +1 charge on the atom?
3
2
4
1
32
True or False: Isomers have the exact same chemical properties.
True
False
33
What does VSEPR theory determine?
Bond length
Bond strength
Bond resonance
Bonding Geometry
34
Which elements is most likely to exhibit an expanded octet in its compounds?
B
Br
C
O
35
Which IMF would hold this substance together as a liquid?
Ion-dipole
Hydrogen bonding
Dipole-dipole
London Dispersion
36
What type of force is holding atoms together in a covalent bond?
van der Waals
Intramolecular
Intermolecular
Ion-Dipole
37
What type of decay do nuclear reactions follow?
quadratic
exponential
progressive
linear
38
Determine the molecular geometry of CH₄
Trigonal planar
Bent
Tetrahedral
Linear
39
What's the main significance of the category trans-uranium elements?
Exist as plasmas
Radioactive
Only exist synthetically
Toxic
40
What type of products are obtained when an acid is added to Na₂CO₃?
Salt & H2(g)
Salt, CO2,& H2O
Salt & H2O
Precipitate
41
What occurs to chloride in the reaction? HCl + NaOH → H₂O + NaCl
Reduced
Neutralized
Oxidized
Spectator ion
42
Determine the molecular geometry of CO₂
Trigonal planar
Linear
Tetrahedral
Bent
43
Reaction Type? Sr(OH)_2(aq) + MgCl_{2 (aq)} → Mg(OH)_2(s) + SrCl_2(aq)
Neutralization
Displacement
Combination
Precipitation
44
Who coined the term radioactivity and identified several new radioactive elements?
Becquerel
Curie
Seaborg
Rutherford
45
When 8 g of NaCl is dissolved into 50 g of H₂O, what is H₂O specifically referred to as?
Solvent
Solute
Colloid
Solution
46
Which of the following is a non-electrolyte?
Li2CO3
NaOH
C2H7N
Ca(NO3)2
47
Which phase of matter do reactions occur fastest?
Occur equally
Liquid
Gas
Solid
48
Which elements are semi-conductive?
Metals
Non-metalloids
Metalloids
Non-metals
49
What type of decay produces an electron?
alpha
delta
beta
gamma
50
T or F: The suction from using a straw allows a beverage to be pushed up by air pressure.
True
False
51
Why is Chlorine more likely to gain electrons than Sulfur ?
Greater number of electron shells
The valence shell is closer to full
The valence shell is closer to empty
Larger effective nuclear charge (Zeff)
52
Who was the first person to show that radioactive elements underwent transmutation?
Becquerel
Rutherford
Seaborg
Curie
53
What type of products are obtained between an an acid and a metal?
Salt, CO2 & H2O
Salt & H2O
Salt & H2(g)
Precipitate
54
Which type of crystals have the lowest melting points?
Molecular
Mettalic
Covalent
Ionic
55
Which gas law shows that the ratio of PV/nT is a constant value?
Ideal gas law
Charles
Avogadro
Boyles
56
Which IMF would hold this substance together as a liquid?
Dipole-dipole
London Dispersion
Hydrogen bonding
Ion-dipole
57
Which elements are malleable solid and a good thermal conductor?
Non-metal
Non-metalloids
Metalloids
Metal
58
Which would generally be the most soluble?
K+
Ni+3
Cr+2
Na0
59
How does a pH 1 solution compare with pH 2? pH 1 is:
2x more acidic
10x less acidic
2x less acidic
10x more acidic
60
What type of products are obtained when an acid is added to a base?
Salt & H2O
Salt, CO2 & H2O
Salt & H2(g)
Precipitate
61
How many pi bonds are found in HCN?
2
1
0
3
62
Reaction Type? Sr(OH)_2(aq) + 2HCl_(aq) → SrCl_2(aq) + 2H₂O_(l)
Combination
Neutralization
Precipitation
Displacement
63
Determine the molecular geometry of NH₃
Bent
Tetrahedral
Trigonal pyrimidial
Trigonal planar
64
A standard is used in which analytical technique to reach the equivalence point?
Titration
Assay
Gravimetric analysis
Extraction
65
Which of the following elements has the greatest electronegativity?
Nitrogen
Selenium
Oxygen
Phosphorous
66
Why is Vanadium is smaller than Calcium?
Larger effective nuclear charge (Zeff)
Greater number of electron shells
The valence shell is closer to empty
The valence shell is closer to full
67
Reaction Type? MgCl₂ + Ca → CaCl₂+ Mg
Displacement
Precipitation
Neutralization
Combination
68
Which pair of properties describe an amorphous solid?
Lacks long-range order / less stable
Lacks long-range order / most stable
Possesses long-range order / less stable
Possesses long-range order / most stable
69
What is the oxidation number of Magnesium in MgCO₃?
0
+2
+4
-1
70
Which type of crystals are held together by electrostatic bonds?
Covalent
Ionic
Mettalic
Molecular
71
True or False: Atoms in an ionic bond will have a small difference in electronegativity.
True
False
72
In what state does the compound K₃PO₄physically exist when dissolved?
3K+ + 2P-3 + 4O-2 (aq)
K3PO4(s)
3K+ + PO4-3 (aq)
K3 + PO4 (aq)
73
Which of the following compounds will have the highest lattice energy?
Na2O
NaF
Na2S
NaCl
74
T or F: Vaporizing a mixture of liquid oil & H₂O will produce a homogenous gaseous mixture.
False
True
75
Which bond type shares electron density directly between the atoms?
Gamma
Pi
Alpha
Sigma
76
If each gas is found at the same temperature, which will have the lowest density?
Equal
He
Kr
Ne
77
What is specifically being exchanged in a precipitation reaction?
Neutrons
Protons
Electrons
Ions
78
Who developed a technique using x-rays to determine the atomic number of an atom?
Henry Moseley
John Newlands
Dmitri Mendeleev
Johann Dobereiner
79
What type of decay produces a helium ion?
gamma
delta
alpha
beta
80
What device is used to measure atmospheric pressure?
manometer
tachymeter
scopometer
barometer
81
Which condition is not an exception to the ideal gas law?
low temperature
High pressure
High density
low mass
82
When 8 g of NaCl is dissolved into 50 g of H₂O, what is NaCl specifically referred to as?
Colloid
Solvent
Solute
Solution
83
True or False: The following are unique isomers.
False
True
84
True or False: As pressure increases, gas particle speed increases.
False
True
85
Which gas law relates volume and temperature?
Ideal gas law
Avogadro
Charles
Boyles
86
Which bond would be the most polar?
Si-S
Si-P
Si-Cl
Si-Si
87
What is the oxidation number of carbon in CH₄?
+4
+3
+6
-4
88
How is the boiling point of water effected at high altitude?
Higher pressure = Higher boiling point
Lower pressure = higher boiling point
Lower pressure = lower boiling point
Higher pressure = Lower boiling point
89
Determine the molecular geometry of BH₃
Trigonal planar
Tetrahedral
Linear
Bent
90
Which is NOT a characteristic of Nuclear reactions?
Nuclear charge is always conserved
Reaction rates are influenced by temperature & concentration
Involve changing of atom identity
Different isotopes influence the reactivity.
91
Which type of crystals are held together by covalent bonds?
Ionic
Mettalic
Molecular
Covalent
92
Which compound has an expanded octet?
BH3
CF4
OF2
SF6
93
Which pH would indicate a basic solution?
5
7
8
6
94
The electron sea theory applies to which type of bonding?
Intermolecular
Ionic
covalent
metallic
95
What is the oxidation number of carbon in CO₂?
+4
+6
-4
+3
96
Determine the molecular geometry of H₂O
Tetrahedral
Trigonal planar
Linear
Bent
97
If each gas is at the same temperature, which will have the lowest average kinetic energy?
Ne
Equal
He
Kr
98
Reaction Type? 2Na + Cl₂→ 2NaCl
Combination
Neutralization
Precipitation
Decomposition
99
Which bond type prevents rotational motion between covalently bonded atoms?
Alpha
Gamma
Sigma
Pi
100
True or False: Isomers have the exact same number of atoms.
True
False
101
T or F: A bed of nails is less dangerous than 1 nail because the greater area reduces pressure
False
True
102
Which IMF would hold this substance together as a liquid?
Hydrogen bonding
Dipole-dipole
Ion-dipole
London Dispersion
103
Which element is most likely to lose an electron?
Barium
Krypton
Calcium
Polonium
104
True or False: The following are identical molecules.
False
True
105
Which element is the smallest?
Selenium
Barium
Polonium
Calcium
106
Which gas law relates volume and pressure?
Boyles
Charles
Avogadro
Ideal gas law
107
What type of decay produces only electromagnetic energy?
gamma
delta
beta
alpha
108
Which one of the following compounds utilizes both ionic and covalent bonding?
Na2O
C2H6O
P2O5
Mg(OH)2
109
What type of force occurs between salt and water in salt water?
Ion-Dipole
hydrogen bond
London dispersion
Dipole dipole

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