Download Chemistry Final

Name:______________________________________________ Date:_________________ Class Period: _____
Chemistry Final 2013 – Semester 1 Review Guide
I.
CLASSIFICATION OF MATTER
1. Define the following:
a. Elements: ___________________________________________________________
b. Compound: _________________________________________________________________
c. Mixture: _____________________________________________________________________
2. What is the difference between homogeneous and heterogeneous mixtures?
3. Identify the following as an element (e), compound (c), or mixture (m):
Substance
E, C or M
As
NaCl
Sand + Water
S
Air
4. State the Law of Conservation of Matter:
5. State the Law of Definite Proportions:
6. Which of the following indicate a chemical change:
(a) Fizzing
(c) Color change
(b) Burning
(d) All of the above
7. Which of the following are physical changes:
(a) State of changes (solid, liquid, gas) (c) Cracking open an egg
(b) Dissolving
(d) All of the above
8. If 30g of KCl are added to 136g of water the resulting mass is _______.
II. LABORATORY SAFETY
1. When should long hair be tied back?
2. When chemicals are spilled what should you do?
III. NUMBERS IN CHEMISTRY
1.
Answer the following calculations to the correct number of significant figures:
a. 3.0 x 2.30 =
____________________________
What’s the rule? _________________
b. 2.3 + 3.44 =
____________________________
What’s the rule? _________________
c. 3.44 x 2.0 + 3.9 ____________________________
2.
3.
4.
Convert the following into scientific notation:
a. 0.0035
____________________________
b. 43,025
____________________________
c. 1
____________________________
d. 0.01
____________________________
Express the following in standard (regular) notation:
a. 3.6 x 104
____________________________
b. 4.9 x 10 - 2
____________________________
How many significant figures do the following numbers have?
a. 0.00321
____________________________
b. 320001
____________________________
c. 1.0000
____________________________
d. .00210
____________________________
5.
There are 60 seconds per minute, 60 minutes per hour, 24 hours per day and 365 days
per year. How many seconds are in a 3 years?
6.
If 3.784 liters = 1 gallon, how many liters are in 4 gallons?
7.
A field goal kicker who makes 20/21 field goals through the center of the uprights has:
8.
What is the formula for density? What is the unit for density? (Draw the density triangle)
(a) poor accuracy but good precision
(b) good accuracy and good precision
(c) poor accuracy and poor precision
(d) good accuracy and poor precision
2
9.
An unknown metal has the mass of 2.5g and a volume of 0.48mL. What is its density?
10.
If the density of a substance is 25g/mL, what is the volume occupied by 300g of the
substance?
11.
Define qualitative and quantitative measurements. Give an example of each.
a. Quantitative measurement:____________________________________________________
b. Qualitative measurement:________________________________________________
12.
What would be the best metric unit for measuring the diameter of a dime?
________________________________________________________________________________
IV. ATOMIC STRUCTURE
1.
What was the contribution to chemistry by each of these individuals?
a. Neils Bohr ___________________________________________________________________
b. Henry Moseley _______________________________________________________________
c. Rutherford ___________________________________________________________________
d. JJ Thomson __________________________________________________________________
e. Schrodinger __________________________________________________________________
f.
Democritous __________________________________________________________________
g. Dalton _______________________________________________________________________
h. Chadwick _____________________________________________________________________
i.
De Broglie ____________________________________________________________________
j.
Millikan ______________________________________________________________________
2.
An atomic number is the same as the number of:
3.
An atom is defined as the smallest part of an element that:
(a)
(b)
(c)
(d)
(a)
(b)
(c)
(d)
Neutrons
Electrons
Alpha particles
Protons
Has protons, neutrons, and electrons
Has protons and neutrons
Retains the chemical identity of that element
Can form an ion
3
4.
The atomic number (# of protons) and mass of chlorine are?
5.
The neutrons of an atom are found:
6.
Which subatomic particle has the smallest mass?
7.
The number of protons always equals the number of __________ in a neutral atom.
8.
The mass number of an element tells you the # of __________ and __________
9.
Who is credited with discovering:
10.
Isotopes have the same number of __________ but different numbers of __________ and
different atomic __________.
(a)
(b)
(c)
(d)
(a)
(b)
(c)
(d)
(a)
(b)
(c)
(d)
17, 35
33, 75
16, 32
29, 64
In the nucleus
Orbiting the nucleus
In the s block
In the orbitals
Protons
Neutrons
Electrons
Ions
a. The nucleus? _______________________
b. The electron? _______________________
c. The Planetary Model of the Atom? _________________________
V. PERIODIC TABLE AND PERIODIC TRENDS
1.
Define these terms AND draw arrows to represent how these trends increase across the
period and within each group:
a. Atomic Radius:
b. Ionization Energy:
c. Electronegativity:
2.
Where can you locate the metals, non-metals, metalloids, alkali metals, alkaline earth
metals, transition metals, halogens and noble gases on the periodic table? (HINT: Draw a
diagram to help!)
4
VI. IONIC AND COVALENT BONDING
1. Naming Ionic Compounds
a. NH4Cl
__________________________________________________
b. Fe(NO3)3
__________________________________________________
c. Cu3P
__________________________________________________
d. Al(CN)3
__________________________________________________
e. Pb(SO4)2
__________________________________________________
2. Formula of Ionic Compounds
a. lead (II) nitride
__________________________________________________
b. silver bromide
__________________________________________________
c. chromium (VI) phosphate
__________________________________________________
d. vanadium (V) sulfide
__________________________________________________
e. potassium bicarbonate
__________________________________________________
3. Naming Covalent Compounds
a. IO2
__________________________________________________
b. C2Br6
__________________________________________________
c. BBr3
__________________________________________________
d. N2O3
__________________________________________________
4. Formula of Covalent Compounds
a. tetraphosphorus triselenide
__________________________________________________
b. disilicon hexabromide
__________________________________________________
c. diselenium diiodide
__________________________________________________
d. tetrasulfur dinitride
__________________________________________________
5. Naming Gases
a. What are the seven diatomic molecules (names and formulas)?
5
VII. CHEMICAL REACTIONS
1. Provide a description and pattern for each type of chemical reaction.
a. Combustion Reaction
b. Synthesis Reaction
c. Decomposition Reaction
d. Single Replacement Reaction
e. Double Replacement Reaction
2. Identify the type of chemical reaction using the following chemical equations. BALANCE.
a. ____ Mg + ____ Fe2O3  ____ Fe + ____ MgO
Type of Reaction: ________________
b. ____ C2H4 + ____ O2  ____ CO2 + ____ H2O
Type of Reaction: ________________
c. ____ PbSO4  ____ PbSO3 + ____ O2
Type of Reaction: ________________
d. ____ H2O + ____ SO3  ____ H2SO4
Type of Reaction: ________________
e. ____ H2SO4 + ____ NH4OH  ____ H2O + ____ (NH4)2SO4
Type of Reaction: ________________
VIII. PREDICTING PRODUCTS AND CHEMICAL REACTIONS
1. Identify the type of reaction, predict the products and write a balanced chemical equation.
a. __Na + __Cl2  ___ __________________
Type of Reaction: __________________
b. ___KI  ___ _______________ + ___ ___________________
Type of Reaction: __________________
c. ___Zn + ___Cu2(SO4)3 ___ ________________ + ___ ____________________
Type of Reaction: __________________
6
d. ___NaOH + ___H2SO4  ___ _______________ + ___ ___________________
Type of Reaction: __________________
e. ___C2H6 + ___O2  ___ ______________ + ___ _____________
Type of Reaction: __________________
2. Definitions
a. Chemical Reaction
_____________________________________________________________________________
b. Balanced Chemical Equation
_____________________________________________________________________________
3. What is always equal on each side of the arrow in a balanced chemical equation?
4. How many atoms are represented in the formula for Cr(CO3)3?
5. Where are reactants and products found in a chemical equation?
IX. PERCENT COMPOSITION (PERCENT BY MASS):
1. What is the equation for percent by mass?
2. What is the percent by mass of each element in CuSO4?
3. What is the percent by mass of each element in H3PO4?
7
X. GENERAL REVIEW
1. Convert the following metric units: (K H D B d c m)
a. 1L =
___________________ mL
b. 100cm =
___________________ m
c. 2735cg =
___________________ g
d. 0.25 KL =
___________________ mL
e. 3.25 g =
___________________ Hg
2. Which SI unit is used to measure:
a. Mass?
___________________
b. Volume?
___________________
c. Length?
___________________
d. Temperature? ___________________
3. In normal processes can total energy be created or destroyed?
4. Label physical or chemical change for the following:
a. A change in color
___________________
b. Phase change
___________________
c. Formation of a new substance
___________________
d. Change in density
___________________
5. Circle ALL the chemical changes below:
a. Burning paper
b. Melting Ice
c. C6H12O6 + H2O  C6H12O6 + H2O
d. Ca + H2O  CaO + H2
6. Identify the following as an element, compound, or mixture.
a. ______________
b._______________
8
c.______________
d.________________
XI. SEPARATION TECHNIQUES
1. Identify the separation technique used in the following:
a. A process used to separate sand and water
______________________________________________________________________
b. An electrical process that can separate water into hydrogen and oxygen gas
______________________________________________________________________
c. Boiling a chemical and then condensing its vapors
______________________________________________________________________
d. A solution is left sitting on the counter. After several days only a solid remains in the container
_______________________________________________________________________
2. Describe the separation technique that could be used to separate each of the following mixtures:
a. Two colorless liquids
_______________________________________________________________________
b. Colored dye or ink
_______________________________________________________________________
c. A non- dissolving solid mixed with a liquid
_______________________________________________________________________
XII. ATOMIC STRUCTURE
1. How do you write a complete chemical symbol for an atom? DRAW A DIAGRAM.
2. If an atom has 14 protons, 15 neutrons and, 14 electrons; its complete chemical symbol would be:
3. If an atom has 8 protons, 8 neutrons, and 10 electrons, its complete chemical symbol would be:
4. If an atom has 13 protons, 14 neutrons, and 10 electrons, its complete chemical symbol would be:
5. If an atom has 11 protons, 12 neutrons, and 10 electrons, its complete chemical symbol would be:
9
6. What is the electron configuration (1s22s2, etc.) for the following atoms:
Long Hand
Noble Gas Conf.
a. Co
________________________________
________________________
b. N
________________________________
________________________
c. Al
________________________________
________________________
d. Ca
________________________________
________________________
e. S
________________________________
________________________
f.
________________________________
________________________
Ar
7. What is the orbital diagram for the following atoms:
a. Fe
b. O
c. N
d. S
e. Be
10