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Chemistry Review for Regents Flashcards | StudBud
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Chemistry Review for Regents
Chemistry Review for Regents
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1
_____ proposed the nuclear structure of an atom (dense positive core, mostly empty space)
JJ Thompson; oil-drop experiment
JJ Thomson; cathode ray experiment
Ernest Rutherford; oil-drop experiment
Ernest Rutherford; gold foil experiment
2
How are the bonds formed in a polar covalent compound?
Electrons are gained.
Electrons are shared equally.
Electrons are shared unequally.
Electrons are lost.
3
How many moles are in 18g of H
2
O?
1
16
18
2
4
1 atm =
101.3kPa
760 mmHg
All of the above
760 torr
5
Which best represents the electron configuration for an atom of iron?
1s2 2s2 2p6 3s2 3p6 4s2 3d6
1s2 2s2 2p6 3s2 3p6 4s2 4d6
1s2 2s2 2p6 3s2 3p6 3d8
1s2 1p6 2s2 2p6 3s2 3p6 4s2
6
What is activation energy?
Minimum energy to transform reactants in activated complex
Minimum energy to transform products in activated complex
Maximum energy to transform products in activated complex
Maximum energy to transform reactants in activated complex
7
Sublimation is
Liquid to gas
Gas to solid
Solid to gas
Solid to liquid
8
_____ states that matter can neither be created nor destroyed.
Charles law
The law of conservation of mass
Dalton's law of partial pressure
Avogadro's number
9
Mono, di, tri, _____, _____, _____
Penta, tetra, hexa
Tetra, hepta, penta
Tetra, penta, hexa
Hepta, tetra, penta
10
Which of the following occurs in an ionic bond?
Like-charged ions attract.
Two atoms share two electrons.
Oppositely charged ions attract.
Two atoms share more than two electrons.
11
Based on the VSEPR theory, what is the molecular geometry of H
2
O ?
bent
pyramidal
linear
tetrahedral
12
Balance to following: _C
3
H
8
+ _O
2
--> _H
2
O + _CO
2
1,2,1,2
2,5,1,3
1,5,4,3
1,3,4,3
13
Which compound contains both covalent and ionic bonds?
H_2O
NaCl
CaCO3
CO2
14
What does a homogenous mixture mean?
All of the above
None of the above
Mixture that has substances are separated by localized areas
Mixture that has the same uniform appearance
15
What are the factors that affect the rates of reactions?
Presence of a catalyst
All of the above
Temperature and concentration
Surface area
16
If the pH of a solution is 7, what is the pOH?
7
0
10
8
17
When a gamma ray is emitted by an element, what happens to the atomic mass and number?
The atomic mass changes, atomic number stays the same.
Atomic mass stays the same, atomic number changes.
Atomic mass changes, atomic number changes.
Atomic mass stays the same, atomic number stays the same.
18
What are the colligative properties?
Vapor pressure lowering
Freezing depression
All of the above
Boiling point elevation
19
What is molar mass ?
mass of a mole of atoms
1 amu
mass of an atom
1 gram
20
Q =
mass
volume
heat
temperature
21
One of the gas law states that:
All of the above
If the P and amount are constant then the T and V are prop.
The total P of gas exerted is equal to the partial P
If the T and amount are constant then the V and P are prop.
22
If the hydrogen ion concentration increases by 100 fold, the pH number will go down by
4
1
3
2
23
What type of reaction is this? C
X
H
Y
+ O
2
→ CO
2
+ H
2
O
Double-replacement
Combustion
Synthesis
Decomposition
24
Which of the following elements does NOT form an ion with a charge of 1+?
Sodium
Potassium
Hydrogen
Fluorine
25
The pH of an acid is _____ while the pH of a base is _____.
Greater than 7; greater than 7
Less than 7; less than 7
Less than 7; greater than 7
Greater than 7; less than 7
26
How many electrons are in the outermost energy level of a neutral atom of aluminum?
8
13
3
2
27
Avogadro’s number is
6.02e23
6.02e22
6.02e25
6.02e24
28
What compound has the chemical formula MgI
2
?
di-iodide magnesium
magnesium(I) iodide(II)
magnesium iodide
iodide(II) magnesium
29
Which one is a compound?
CH_4
O_2
Re
Tm
30
What is a n Arrhenius acid?
liberates an H+ ion in solution
Proton receiver
Electron donor
Neutron donor
31
pH determines
molarity
H+ ion concentration
solubility
OH- concentration
32
Equilibrium can shift depending on
Changing in temperature
Increasing products
All of the above
Increasing reactants
33
A hydrogen atom is essentially a(n)...
Electron
Neutron
Proton
Nucleus
34
Which element has 8 valence electrons?
Potassium
Helium
Oxygen
Neon
35
Exothermic is the process of _____ and endothermic is the process of _____.
Energy intake; energy release
Energy release; energy intake
Energy release; energy release
Energy intake; energy intake
36
A reactant is a substance in a chemical reaction that is ______
on the left side of the arrow
created
on the right side of the arrow
destroyed
37
% composition can be found in what way?
m/m
m/v
All of the above
m/mol
38
Molarity is…
Mass of solute/mass of soln
Moles of solute/Kg of solvent
Mass of solute/100 mL of soln
Moles/Liters of soln
39
Polyatomic ions…
Include ammonium
Are a group of atoms that have a charge
All of the above
End in “ate” or “ite”
40
NEVER look at the periodic table for the charges of:
Transition metals
Covalent compounds
Ternary ionic compounds
Binary molecular compounds
41
Which occurs if an electron transitions from PEL= 5 to PEL = 2 in a hydrogen atom?
Energy is released, and visible light is not emitted.
Energy is released, and visible light is emitted.
Energy is absorbed, and visible light is not emitted.
Energy is absorbed, and visible light is emitted.
42
Matter is _____, and energy is _____.
Cycled; transferred
Transferred;cycled
Transfered;transferred
Cycled; cycled
43
Molecular formulas _____.
Give # of atoms of each element in a molecule of a compound
have the smallest positive integer ration
None of the above
Regular formulas
44
Le Chatelier's principle states that when a system at equilibrium placed under stress:
The system will increase and relieve stress as an equal rate
It will undergo a change in such a way as to relieve stress
The system will undergo no change
It will undergo a change in such a way as to increase stress
45
What is the ideal gas law?
V1/T1 = V2/T2
PV = nRT
P x T = P x 1 + Px 2 + Px3…
P1/T1 = P2/T2
