Chemistry Practice Final Exam Flashcards

Terms Definitions
Atoms cannot be:
Atoms have a possitive charge.
B) 932 mg = ____ g

This greek philosipher had the idea that all matter was made of tiny parts:
Are atoms made up of smaller parts?
A) 6.85 m = ____ cm
0.0685 cm

What are is all matter made up of?
Atomic Mass
The total number or protons and neutrons in the nucleus of an atom:
How mant electrons can the "M" shell hold?
If there are 5 protons how many electrons are there?
John Dalton
The atomic theory was based upon his ideas:
A part of an atom with a positive charge:
Two or more atoms with the same atomic number but different atromic masses:
Chemical Changes
What happens when atoms link up or seperate from each other?
10. The most penetrating form of radiation is ____________.
a) alpha radiation b) beta radiation c) gamma radiation
d) a, b, & c are all the same e) a & b
c) gamma radiation
22. Based on its position in the Periodic Table, which of the following is the most probable charge of a
magnesium ion?
a) -2
b) -6
c) +1
d) +2
e) +3
d) +2
16. In the reaction given, how many moles of I2 are needed to react with 1.2 mol of Al?
2 Al + 3 I2 -> 2 AlI3
a) 0.60
b) 1.2
c) 1.8
d) 2.4
e) 3.6
c) 1.8
A part of an atom that has a negative charge:
1. Which pair of elements is most likely to form an ionic compound if allowed to react together?
a) Al & I
b) Cu & Ca
c) C & Cl
d) P & Br
e) K & Ni
a) Al & I
Which has the greater ionization energy? (barium or magnesium)

The energy required to remove an electron from an isolated atom.
-Reading down a group, the ionization energy decreases, because of the atom's size increases. The outermost electron is progressively farther from the nuclear charge, hence easier to remove.
-Reading across a period, the ionization energy increase, note that atomic size decreases, because the outer most electrons are close to the nucleus, thus harder to remove.
4. The metric unit used to measure mass is the ________.
a) gram, g
b) grams per cubic centimeter, g/cm3 c) Kelvin, K
d) liter, L
e) meter, m
a) gram, g
26. In the reaction, CO32- + H2O <-> HCO31- + OH1-, the CO32- ion is acting as a(n) _____.
a) Arrhenius acid
b) Arrhenius acid
c) Bronsted-Lowry acid
d) Bronsted-Lowry base e) none of these
d) Bronsted-Lowry base
25. What happens to the pressure of a gas inside a container if the temperature of the
gas is lowered? The pressure _____.
a) increases b) does not change c) decreases
c) decreases
13. Consider the reaction shown and identify the statement that is true.
CaCO3(s) (heat)/-> CaO(s) + CO2(g)
a) This reaction is balanced as written. b) Heat is required for this reaction to occur.
c) The products are a solid and a gas. d) Th
e) All of these.
7. Which factor(s) would increase the rate of a reaction?
I) increasing the temperature II) increasing the concentration of reactants III) adding a catalyst
a) I & II only b) II & III only
c) III only
d) I & III only
e) I, II, & III
e) I, II, & III
2. Which of the following is a property typical of ionic compounds?
a) exist as crystalline solids at room temperature
b) conduct electrical current if dissolved in water or melted
c) have very high melting points and boiling points
d) are hard and brittl
e) all of these
30. Which of the following is a characteristic of bases?
a) turn litmus blue b) feel slippery c) taste bitter
d) neutralize acids e) all of these
e) all of these
14. Which statement concerning Arrhenius acid-base theory is correct?
a) An Arrhenius acid produces hydrogen ions in water solution.
b) An Arrhenius base produces hydroxide ions in water solution.
c) A neutralization reaction produces water and a salt.
e) All of the above are correct.
7. If the temperature of a fixed volume of a gas is increased, what effect will this have on the
pressure of the gas?
a) The pressure will increase. b) The pressure will decrease.
c) The pressure will be unchanged.
d) The pressure will increase and
a) The pressure will increase.
1. The solubility of gases in liquids is highest at _____________________.
a) low temperature and high pressure
b) low temperature and low pressure
c) high temperature and high pressure
d) high temperature and low pressure
a) low temperature and high pressure
15. How many moles of NaCl are in 4.86 g of NaCl?
a) 0.0831
b) 2.93 x 1024
c) 4.86
d) 284
e) 12.0
a) 0.0831

Use conversion traingle
6. Which of the following is a part of the kinetic theory of gases?
a) Gas particles are in constant, rapid motion.
b) There are no attractive forces between gas particles.
c) The distance between gas particles is very large.
d) The collisions between gas
e) All of these
14. Which elements all belong in the same group?
a) N, O, F
b) Fe, Co, Ni
c) B, Si, As
d) Na, K, Cs
e) Al, Ge, Sb
d) Na, K, Cs

group is vertical roll
7. Which of the following regions of the electromagnetic spectrum has the highest energy?
a) ultraviolet light b) infrared light
c) radio waves
d) red light
e) gamma rays
e) gamma rays

high to low
Gamma rays, X-ray, ultraviolet light, visible light, infrared light, microwaves, radio waves
14. What is the mass of 0.255 mol of K?
a) 0.255 g
b) 39.1 g
c) 9.97 g
d) 7.91 g
e) 153 g
c) 9.97

use the conversion triangle
12. When a reaction system is at equilibrium, _____.
a) there is no more chemistry happening
b) the amounts of reactants and products are exactly equal
c) the reaction rate in the forward direction is at a maximum
d) the reaction rate in the reverse direc
e) the rates of the forward and reverse directions are exactly equal.
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