Semester 1 Final Review Sheet
Unit 1 – Introduction to Matter
Dimensional Analysis
1. 691 mm = ________km
2. 99 km = ________dm
Mole Conversions
5.7 moles of O2 gas = _____ liters of O2 gas
9 L of He gas = _____ moles of He gas
Significant Figures
.0050
5005
.005
5000
45.45 + 59.595 + 26.35
8000 x 15
Measurements
State the current measurement for the ruler below
Accuracy and Precision
If we were trying to get a reading of 5.25, and got 5, 5.5, 5.35, 5.15 would you say this was accurate or precise,
why?
If we were trying to get a reading of 3.1 and we got 4.2, 4.18, 4.22, 4.19, and 4.21 would you say this was
accurate or precise, why?
Physical Properties and Changes
Chemical Properties and Changes
Law of conservation of Matter
Define Density:
Draw a picture of each of the forms of matter:
Give an example of each of the following:
Element
Compound
Heterogeneous Mixture
Homogeneous Mixture
Label the various states of matter and various phase change processes:
Unit 2 – Atomic Theory
Explain how the following experiments changed atomic theory:
a. Gold Foil Experiment
b. Cathode Ray Tube Experiment
Define Isotope:
What determines the atomic number of an element?
What determine the mass number/atomic mass of an element?
Label the following for the following element:
Name:
Symbol:
Atomic Number:
Mass Number/Atomic Mass:
Fill in the following table on subatomic particles:
Substance
Symbol
Ytterbium
Potassium
Yb
K
Atomic
Number
Mass Number
Number of
Protons
Number of
Neutrons
47
106
32
88
16
50
Determine both the number of valence electrons and occupied shells for the following elements:
Valence Electrons
Number of occupied shells
Beryllium
Aluminum
Fill in the missing information for electron configuration
Si _____ Period___
Mg _____ Period___ 2.8.1 ___ Period___
2.5___ Period___
Draw the four atomic models (Dalton, Thomson, Rutherford, and Bohr) and label the protons,
neutrons, electrons, and nucleus if present.
Draw the Bohr model of Sulfur
Calcium
Unit 3 – Chemical Relationships
Identify the three types of substances on the periodic table, their general location, and their properties:
How many valence electrons would elements in the following groups have:
1:
2:
13:
14:
15:
16:
17:
18:
State the octet rule:
Label how electronegativity and atomic radius change:
Identify the column number of each of the following elemental families:
Alkali Metals
Alkaline Earth Metals
Halogens
Noble Gases
What charge of ion will elements in the following groups have:
1:
2:
13:
14:
15:
16:
17:
18:
Type of Bond
Structure
Ionic
Covalent
Metallic
Melting/Boiling Conductivity Water
Soluble?
Alcohol
Soluble?
NA
NA
NA
What are the two special properties that only metals have:
Substance does not conduct electricity when dissolved in water, has a low melting point, and is crystalline and
brittle:
Substance conducts electricity when dissolved in water, is crystalline, and brittle:
Substance dissolves in alcohol, is crystalline and brittle:
Substance dissolves in water, and has a high melting point:
Ionic Naming
Na2CO3 ____________________________________________________
NaOH _____________________________________________________
Ionic Formula Writing
Sodium Nitrate
Lead (II) Sulfide
__________
__________
Lead (IV) Phosphide
Iron (II) Oxide
Lewis Structure Ionic Bonding
Potassium and Bromine
__________
__________
Silicon and 2 Sulfur
Covalent Naming
SO3
____________________________________________
SiCl4
____________________________________________
Covalent Formula Writing
Silicon disulfide
Sulfur dioxide
__________
__________
Diboron monosulfide
Xenon hexafluoride
Lewis Structure Covalent Bonding
Fluorine and Fluorine
Arsenic and 3 Iodine
__________
__________