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Physical Science- First Semester Exam 2015-2016 KEY
What will your exam consist of?
o
o
100 multiple choice questions over course content & laboratory assignments
Problems on atomic structure, equation balancing, formula mass calculation, formula writing
ion formation and drawing structural formulas
What can you bring to your exam?
o Pencils
o Calculator
o Prepared 3 X 5 notecard
 Must be handwritten
 Both sides can be used
 You may put anything you want on this notecard.
Atomic structure
A) Subatomic particles
a. What are the atomic mass units for protons, neutrons, and electrons? Protons and
neutrons = 1 amu; electrons about 0 amu
What does the atomic number represent? # of protons
b. What does the mass number represent? # of protons + # of neutrons
c. What particles are in equal numbers in a neutral atom? Protons and electrons
d. How is the number of protons determined? From the atomic number
e. How is the number of neutrons determined? Mass # - # of protons
f. How is the number of electrons determined in a neutral atom? # protons = # electrons
g. What subatomic particles are located in the nucleus? Protons and neutrons
h. Complete the following diagrams and fill in the charts for each element. Use the periodic
table as a reference.
5
5
6
11
2-3
------------------------------------------------------------------------------------------------------------------
10
10
10
20
2-8
1
C) The electron cloud
a. What determines the location of an electron in the electron cloud? How many energy
levels are present. Electrons fill the energy levels in order (2-8-8-18)
b. How many electrons can be found in the first energy level of an atom? 2
c. How many electrons can be found in the second energy level of an atom? 8
d. How can the electron arrangement/configuration be determined for a neutral atom? In a
neutral atom the # of protons = # electrons then fill energy levels using the following
arrangement 2-8-8-18
D) Isotopes
a. How are isotopes different from other forms of the same element? They have the same
number of protons but different number of electrons and mass number.
b. Which pairs of atoms are isotopes of the same element?
i.
ii.
16
8O
and
122
50Sn
iii.
39
17Cl
iv.
121
50Sn
17
8O
and
and
122
52Te
39
19K
and
119
50Sn
c. Identify the most abundant isotope for each element.
i. Fe-54 Fe-56 Fe-57 Fe-58
ii. O-16 O-17 O-18
iii. Mg-24 Mg-25 Mg-26
iv. S-32 S-33 S-34 S-36
v. Ar-36 Ar-38 Ar-40
vi. Hg-196 Hg-198 Hg-199 Hg-202 Hg-204
vii. Kr-78 Kr-80 Kr-82 Kr-83 Kr-84 Kr-86
Periodic Table
A) Identifying elements by atomic number
a. Atomic # is the number of? protons
B) Identifying elements with the same number of valence electrons (which column?)-see first periodic
table below
a. Which elements have one valence electron? Group/Family 1
b. Which elements have two valence electrons? Group/Family 2
c. Which elements have three valence electrons? Group/Family 13
d. Which elements have four valence electrons? Group/Family 14
e. Which elements have five valence electrons? Group/Family 15
f. Which elements have six valence electrons? Group/Family 16
g. Which elements have seven valence electrons? Group/Family 17
h. Which elements have eight valence electrons? Group/Family 18
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C) Identifying elements by family
a.
b.
c.
d.
Which
Which
Which
Which
elements
elements
elements
elements
are alkali metals? Group/Family 1
are alkaline earth metals? Group/Family 2
are halogens? Group/Family 17
are noble gases? Group/Family 18
D) Identifying elements by period (which row?)
a.
b.
c.
d.
e.
f.
g.
Which
Which
Which
Which
Which
Which
Which
elements
elements
elements
elements
elements
elements
elements
have
have
have
have
have
have
have
one electron shell? Period 1
two electron shells? Period 2
three electron shells? Period 3
four electron shells? Period 4
five electron shells? Period 5
six electron shells? Period 6
seven electron shells? Period 7
E) Identifying elements by area of the periodic table
a. Which elements
b. Which elements
c. Which elements
d. Which elements
Periodic table
are metals? Blue
are nonmetals? Yellow
are metalloids? Pink
are transition metals? Purple/pink in top
Using the Periodic Table, give the following information for the element Nitrogen:
_____7______1. Number of protons
_____7______2. Number of neutrons
_____5______3. Number of valence electrons
_____2______4. Number of electron shells
___nonmetal__5. Metal or non-metal?
_____O______6. Symbol of the element with the next highest atomic number
_Group/Family 15_7. Name of the chemical family containing Nitrogen
_P,As,Sb,Bi__8. Name of another element in the same family with Nitrogen
_Li,Be,B,C,O,F,Ne____9. Name of another element in the same period with Nitrogen
Ionic bonding
A) Electrons are transferred between atoms
B) Valence electrons- outer shell electrons
C) Metals
a. Lend valence electrons
b. 1 – 4 valence electrons
c. Form positive ions ( more protons than electrons) cation
D) Nonmetals
a. Borrow valence electrons
b. 4 - 8 valence electrons
c. Form negative ions (more electrons than protons) anion
E) Metals lend and non-metals borrow to become stable.
a. Stable- having only full outer electron shells
F) Oxidation number
3
a. The number of electrons an atom can lend, borrow, or share
b. Metals have positive oxidation numbers
1. Calcium has two outer shell electrons
2. Calcium lends two electrons
3. Calcium has an oxidation number of 2+
c. Nonmetals have negative oxidation numbers
1. Oxygen has six outer shell electrons
2. Oxygen gains two electrons to have a full outer shell of 8
3. Oxygen has an oxidation number of 2d. There are no oxidation numbers above 4.
G) Electrolytes
a. Ionic compounds dissolved in water will conduct electricity
H) Draw the electron configuration for the following:
a. Potassium
c. Aluminum
b. Lithium
d. Carbon
I) Draw the ionic bonds between the following. Make sure to draw the Lewis Dot structures. Which
ones are the anions and cations:
a. Sodium & Phosphorus
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b.
Lithium & Chlorine
J) Draw the electron dot diagram (Lewis Dot Structure) and then tell if it would give up or take on
electrons to get a full shell. Also tell what charge it would have (positive or negative and how much
ex: +2)
Rules for formula writing
A) Metals are listed first
B) Nonmetals are listed second
C) The total number of electrons shown as being lost by the metal must equal the total number of
electrons shown being gained by the nonmetal.
D) The number 1 is NOT used as a subscript.
E) When the subscripts would be the same for both the metal and nonmetal they are not used.
F) Examples
a. Calcium and Chlorine- CaCl2
b. Magnesium and oxygen- MgO
c. Magnesium and phosphorus- Mg3P2
G) Write the formulas for the following compounds.
1. Magnesium chloride _____MgCl2__________
2. Magnesium nitride ______Mg3N2____________
3. Copper (II) nitride ______Cu3N2___________
4. Titanium(III) oxide _____Ti2O3___________
H) Write the correct formula for each of the following compounds.
1) Cesium fluoride (cesium & fluorine) CsF
4) Strontium nitride (strontium & nitrogen) Sr3N2
2) Potassium oxide (potassium & oxygen) K2O
5) Aluminum bromide (aluminum & bromine) AlBr3
3) Rubidium nitride (rubidium & nitrogen) Rb3N
6) Aluminum iodide (aluminum & iodine) AlI3
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Types of chemical reactions
Synthesis
A+B
Decomposition
AB
AB
A+B
Single Replacement
Double Replacement
AB + C
AB + CD
CB + A
CB + AD
Tell what kind of reactions are the following (synthesis, decomposition, etc):
a. CaCl2 + Na2CO3  CaCO3 + 2NaCl ______double replacement___________
b. HC2H3O2 + NaHCO3  NaC2H3O2 + H2O + CO2 __decomposition___
c. NaCl  Na + Cl2 ___decomposition___________
d. NaOH + HCl  H2O + NaCl ___double replacement____________
e. K + Cl2  KCl _____synthesis______________
f. K + AgCl  Ag + KCl _____Single Replacement_________
g. KOH + HNO3  H2O + KNO3 __double replacement________________
h. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4 _double replacement__________________
i.
Na2O + CO2  Na2CO3 _____synthesis______________________
j. Pb(NO3)2 + 2HCl  2PbCl2 + 2HNO3 ____double replacement____________
k. Ca + 2HCl  CaCl2 +H2 ____single replacement______________
Components of a chemical reaction
A. Matter
a. Identify products in a chemical equation
b. Identify reactants in a chemical equation
c. Reactants
Products
B. Energy
Exothermic reactions
 More energy is released than is
needed to continue the reaction
 Reactants have more
energy than products
 Energy is released to the
surroundings
 Would feel warm
Endothermic reactions
 Less energy is released than
is needed to continue the reaction
 Products have more
energy than reactants
 Energy is absorbed
from the surroundings
 Would feel cold
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A) What types of reactions involve breaking of chemical bonds and heat being released?
___exothermic_
B) The exothermic reaction has energy __released_ by the reaction.
C) The endothermic reaction has energy ____absorbed______ by the reaction.
D) This reaction is cold to the touch. ____endothermic_____
E) This reaction is warm/hot to the touch. __exothermic_______
Law of Conservation of Mass
A. In a chemical reaction mass is neither lost nor gained.
a. Atoms are rearranged
b. Equations are balanced to show Conservation of Mass
B. For the equation below, put a circle around the subscripts and a square around the coefficients.
C. Calculate the formula mass for the following compounds. Show your work in the correct format.
1) Al2(SiF6)3
Al
Si
F
Number of
atoms
2
3
18
2) (NH4)2S2O3
Mass
number
27
28
19
54
84
342
N
H
S
O
Number of
atoms
2
8
2
3
Mass
number
14
1
32
16
480 amu
3) 2Al2(SiF6)3 =
28
8
64
48
148 amu
____960 amu____
Reaction rate
A. Substances must collide to react
B. The more collisions the faster the reaction
C. Four factors that affect reaction rate
a. Surface area- amount of exposed surface
b. Temperature- affects how fast particles move
c. Catalysts- affect reactions without being part of the reaction
d. Concentration- how much of a material is in a given area
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Flame tests- results
A. Oxygen- Splints re-light
B. Carbon dioxide- Splints go out
Phase Changes- On the diagram below label solid, liquid, gas, melting, evaporation, condensation, freezing.
(B and D have two answers) Write right on the diagram.
States of Matter
Fill in the table below
State of matter
Volume
Shape
Movement of
Particles
Space Between
Particles
Fixed
Fixed
Vibrates
Very close together
Unfixed
Moves faster and
particles can flow
past each other
Further apart
Unfixed
Moving very fast
Very far apart
Solid
Liquid
Fixed
Gas
Unfixed
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Determine if the following is a chemical or physical properties:
_P_1. Oxygen is odorless and colorless
_C_2. Copper turns green when exposed to the environment
_P_3. The piece of metal is magnetic
_P_4. The density of water is 1.0 gram per cubic centimeter
_P_5. Diamonds are a very hard substance
_P_6. The tree is 8 meters high
_C_7. Sodium reacts very easily with other elements.
_P_8. Copper conducts electricity
_P_9. Nitrogen is a colorless gas
_C_10. The silver spoons tarnished and turned dark
Determine if the following is a chemical or physical changes:
_C_1. Milk sours.
_P_2. An apple is cut.
_P_3. Sugar dissolves in water.
_C_4. Grass grows.
_P_5. Heat changes H2O to steam.
_C_6. Food is digested.
_P_7. Alcohol evaporates.
_P_8. Ice melts.
_C_9. Wood rots.
_P_10. Paper towel absorbs water.
Classification of Matter
i.
Match each diagram with its correct description. Diagrams will be used once.
A
1.
2.
3.
4.
5.
ii.
B
C
D
E
_C__ Pure Element – only one type of atom present.
_E__Mixture of two elements – two types of uncombined atoms present.
_B__Pure compound – only one type of compound present.
_A__Mixture of two compounds – two types of compounds present.
_D__Mixture of a compound and an element.
Column A lists a substance. In Column B, list whether the substance is an element (E), a
compound (C), a Heterogeneous Mixture (HeM), or a Homogeneous Mixture (HoM).
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Column B
Column A
1. Steam (H2O)
2.
Salt Water (NaCl & H2O)
3. Pencil lead (C)
4. Dirt
5. Pepsi
6. Silver (Ag)
7. A burrito
8.
Italian Dressing
9. Chicken Soup
10. Lemonade with pulp
C
HoM
E
HeM
HoM
E
HeM
HeM
HeM
HeM
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