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1. Hypothesis
2. Conclusion
3. Data
4. Liquid
5. Gas
6. Scientific Method
7. SI Units
8. Mass
9. Volume
10.Density
11.Significant Figures
12.Fahrenheit
13.Celsius
14.Matter
15.Compound
16.Solution
17.Mixture
18.Units
19.Periodic Table
20.Atomic Mass
Unit(AMU)
21.Element
22.Group
23.Period
24.Ions
25.Isotopes
26.Electrons
27.Protons
28.Neutrons
29.John Dalton
30.Atoms
31.Fusion
32.Fission
33.Malleability
34.Ductility
35.Luster
36.Metalloid
37.Cation
38.Anion
39.Acid
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Step of the Scientific Method
A physical state
A unit of measurement, the metric system
Length* Width* Height
Mass/Volume
SAE unit of temperature
SI unit of Temperature
Number of numbers past the decimal
A substance that can be broken down
A homogenous mixture in aqueous suspension
Unit of measurement for measuring mass of
elements
The name of columns on the periodic table
The name of rows on the periodic table
The electronic charge of an atom
All elements in order
A unit of energy
Positive or negative charge on an atom or
group of atoms
Atoms of the same element with different
atomic mass
A negatively charged particle
A positively charged particle
An atomic particle with no charge
Used Boyle’s information to create the atomic
theory
The smallest atomic unit
The process of combining two light nuclei to
form a heavier more stable nucleus
The process of using a neutron to split a heavy
nucleus into two nuclei with smaller mass
numbers
Brittle versus soft
Stretchable
Metal-like but does not contain all metal
characteristics
A positively charged particle
A negatively charged particle
Substance which produces hydrogen ions in
aqueous solution, proton donor
Not printed, Answer not present
1
T/F
Mark a T for True statements and F for False statements
40.Most materials occur in nature as pure substances.
41.Atoms are made up of tiny particles called molecules.
42.Atoms are not created or destroyed in chemical reactions. A chemical
reaction simply changes the way atoms are grouped together.
43.The nucleus of an atom contains the electrons and the neutrons.
44.A proton is equal to one atomic mass unit and has a positive electrical
charge.
45.An electron is held near the nucleus due to an attractive force.
46.A physical property of a Cu is that it is malleable.
47.A physical property of Se is that it has luster.
48.A physical property of Br is that it conducts electricity.
49.An ionic charge between a metal and a non metal has a net charge of
zero
50.PbO2 is Plumbic Oxide
51.N2O5 is dinitrogen pentoxide.
52.HNO2 is nitrous acid.
53.HC2H3O2 is acetic acid
54. An ion with one more electron than a proton is said to have a
negative charge.
55. The elements of Group 7 are said to have a charge of +1.
56. A polyatomic compound has at least three or more elements.
57. When balancing a chemical equation, one must never change the
coefficient of any reactant or product.
58. The atomic number (Z) represents the number of protons in the
nucleus.
59. AMU stands for Atomic Mass Unit.
Multiple Choice Mark the most correct answer.
For the following elements, complete the following—
Element
Symb
ol
Potassium
60.
# of
proton
s
61.
# of
Neutron
s
62.
2
# of
Electron
s
63.
Atomi Perio
c Mass d
Grou
p
64.
66.
65.
67. An example of a Type 2 cation is
68. A noble gas is
69. The element Cl has _________ number of positive valence electrons
70. Use the elements Li and N to create a balanced ionic compound.
71. Which of the following is not a Type 1 compound?
72. Name a Type 1 Compound?
73. Name a Type 2 compound?
74. Name a Type 3 Compound?
75. Name an Acid?
76. Does and Acid contain a Hydrogen ion or a hydroxide ion?
77. CO3- is called
78. The substances used in a chemical equation are called _____________
and the substances present after the reaction are called
__________________
79. If Calcium Carbonate is heated strongly, Carbon Dioxide is driven off,
leaving a residue of Calcium Oxide. Write an unbalanced equation.
Balance the equations, identify the coefficients
80.
______H2O2 (aq)  _____H2O (l) +______O2 (g)
81.
______CaF2(s) + _____H2SO4(l) ______CaSO4$(s) + _____HF (g)
82.
______ C5H12(l) + ______O2(g)  _______CO2(g) + _______H2O(g)
83. _____MnO2(s) + ____ HCl(aq)  ____MnCl2(aq) + _____Cl2(g) +
____H2O(l)
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