Honors Chemistry Summer Assignment
The goal of this summer assignment is to review information that was
previously covered in middle school and 9th grade to adequately prepare
you for the rigor of honors chemistry. This class is fast-paced and the
honors chemistry teachers expect that you are entering class prepared from
the first day.
Each topic covered has associated links listed with it. If you need a
refresher on any of the material, these links are where you should begin.
We highly recommend that you take formal notes from these links as they
will serve as your class notes for the year on the selected topics.
The summer assignment is due on the first day of class: September
2,
2015
Please come to class with your completed summer assignment and any
questions you may have on the material covered.
Look forward to seeing you in class!
Section I – Matter & Properties
Matter & Properties, Part I: https://www.youtube.com/watch?v=TF8rxXs-QSY
Matter & Properties, Part II: https://www.youtube.com/watch?v=WGhGcrTVDVI – through 7:00
Classifying Matter, Part I: https://www.youtube.com/watch?v=ZZYjleLadlc
Classifying Matter, Part II: https://www.youtube.com/watch?v=SoFywULNF3s
Chemical Reaction Basics: https://www.youtube.com/watch?v=9Jpr8UoDOj0
1. Classify each of the following as either an intensive (I) or extensive (E) property.
Water’s density is 1.0 g/mL
Grass is green
I
E
Metal conducts heat
I
Boiling point is 100°C
I
A cup has 500 mL of water
E
I
A stone weighs 10 lbs.
2. Fill in the following concept map for the classification of matter:
Classify each of the following as an element (E), compound (C), heterogeneous mixture (HE), or homogeneous
mixture (HO).
Sodium chloride
__C___
Concrete
_HE____
Air
HO
Water
__C___
Salad
_HE____
Lead
14-carat gold
__HO___
Oxygen
__E___
Kool-Aid drink
E___
HO
Classify each of the following as either a physical (P) or chemical (C) property.
Ice melts at 0°C _P__
Copper conducts electricity __P___ Getting tan in sun
__C_
Iron rusts
Iron is magnetic __P_
__C_
The sky is blue
__P___ The gas is colorless
_P___
Baking a cake
__C___ Density is 1 g/cm3
__P_
3. List the 5 signs of a chemical reaction:
a. _____bubbling/gas released________________
b. _____color change_______________________
c. ____heat absorbed or released_____________
d. ____precipitate formation when mixing two liquids or solutions
e. _____change in physical properties_________
Section II: Chemical Math
LINKS:
Density: https://www.youtube.com/watch?v=4fUJQiLhfhU
SI Units: https://www.youtube.com/watch?v=WuaxXcgX6Rc
Metric Units: https://www.youtube.com/watch?v=5EcNAxweb44 (through 5:05) Dimensional
Analysis: https://www.youtube.com/watch?v=WrIOeKtqNz8
12. Simple density problems:
a. Determine the density of an object with a mass of 13.25 g and occupies of volume of 3.7 cm3.
13.25𝑔
3.7𝑐𝑚3
= 3.6g/cm3
b. Gold has a density of 19.30 g/cm3. What is the mass of a piece of gold that has a volume of 5.35
cm3?
19.30g = 1 cm3 for gold
19.3𝑔
𝑥
=
x = 103g
5.35cm3 x 19.30g = 103g
1 𝑐𝑚3 5.35𝑐𝑚3
1 cm3
c. What is the volume of a piece of aluminum with a density of 2.70 g/cm3 and a mass of 415 g?
415𝑔
𝑥
=
2.70𝑔
1𝑐𝑚3
x = 154cm3
2.70g = 1 cm3 for aluminum
415g x 1 cm3 = 154cm3
2.70g
4. Fill in the following table depicting the SI units:
Type of Measurement
Units (words)
Units (symbol)
amount of substance
mole
mol
mass
kilogram
kg
temperature
Kelvin
K
time
second
s
Length
meter
m
5. Fill in the following table depicting metric prefixes:
giga
mega
kilo
deci
centi
milli
micro
nano
pico
G
M
k
d
c
m
µ
n
p
109
106
103
10-1
10-2
10-3
10-6
10-9
10-12
**Memorize highlighted units
6. Use dimensional analysis to solve the following questions.
** purple answers are rounded with the correct number of significant figures. We will cover this later
in the unit.
a. 35.0 grams to decigrams
35.0g x 101 dg = 350 dg
1g
(350. dg)
b. 16.4 pounds to grams (1 kg = 2.2 lbs)
16.4 lb x 1 kg x 103g = 7455g
2.2 lb 1 kg
(7460g)
1 month to seconds (assume that 1 month = 30 days)
30 days x 24 hr x 3600 sec = 2,592,000 sec (2.592 x 106 sec)
1 day
1 hr
c.
(3 x 106 seconds)
2.8 days to milliseconds
2.8 days x 24 hr x 3600 sec x 103 msec =
1 day
1 hr
1 sec
241,920,000 msec (2.4192 x 108 msec)
(2.4 x 108 msec)
Section III: The Atom
LINKS:
Democritus & Dalton: https://www.youtube.com/watch?v=gmwgJ6bDLHM
Thomson – Rutherford: https://www.youtube.com/watch?v=4Gymoej6N2A
Structure of Atom: https://www.youtube.com/watch?v=9l1HZwn2tOA
Bohr: https://www.youtube.com/watch?v=CUk3enr-m0w
Heisenberg – Schrödinger: https://www.youtube.com/watch?v=cy2rEt63Af4 – until 3:50
7. Fill in the chart below. This will be your reference for the history of the atom as we progress through
the year.
Main Ideas
Scientist
Experiment
Sketch of Model
Democritus
400 BC
All matter is made of indivisible
particles called “atomos”.
Dalton
1800s
Father of Modern Atomic Theory
1. All matter is composed of atoms
2. All atoms of a given element are
identical
3. Atoms can’t be created, subdivided
or destroyed
4. In a chemical reaction atoms can
combine to form compounds
5. Atoms of different elements can be
distinguished from one another by
mass
(1897) Discovered that cathode rays are
composed of negatively charged
particles with a large charge/mass ratio
(discovered electrons)
Thomson
Cathode ray
experiments
https://www.youtube.
com/watch?v=O9Go
yscbazk
Millikan
Measured the charge of an electron
(1909)
Oil drop experiment
https://www.youtube.
com/watch?v=XMfY
Hag7Liw
Rutherford
Atoms are mostly empty space, with a
small, positively charged nucleus.
(1910)
1917 – discovers protons
1921 – hypothesizes presence of
neutrons
Gold Foil
Experiment
https://www.youtube.
com/watch?v=5pZj0
u_XMbc
Bohr
Described specific behavior and position
of electrons; electrons travel in fixed
orbits at set distances from the nucleus.
The amount of energy each electron has
is determined by which orbit it is in.
(1913)
Studied spectrum for
hydrogen; his
equations only work
for hydrogen
Heisenberg
Uncertainty Principle (1926)
It is impossible to know both the
position of a particle and its
speed/direction at the same time.
Not necessary, (or
Heisenberg’s
experiment) but
good link explaining
the Uncertainty
Principle further if
you are curious:
https://www.youtube.
com/watch?v=a8FTr
2qMutA
Schrödinger
Quantum Mechanical Model of the
atom; series of equations describing the
clouds where there is a high probability
of finding the electron in the atom
(1926)
8. Fill in the table below for the various atoms.
NAME
SYMBOL ATOMIC
MASS
PROTONS ELECTRONS NEUTRONS
NUMBER NUMBER
Lithium
Li
3
7
3
3
4
Lead
Pb
82
207
82
82
125
Manganese
Mn
25
55
25
25
30
Nickel
Ni
28
59
28
28
31
Mercury
Hg
80
202
80
80
122
Tungsten
W
74
187
74
74
113
Iodine-131
131
I
53
131
53
53
78
U
92
236
92
92
144
56
141
56
56
85
Uranium-236
236
Barium-141
141
Ba
9. Atoms are neutral, meaning that the number of protons equals the number of electrons. Atoms that have
charges are called ions. Positive ions mean that electrons have been lost. Negative ions mean that
electrons have been gained. Use this information to fill in the chart below.
NAME
SYMBOL ATOMIC
MASS
PROTONS NEUTRONS ELECTRONS
NUMBER NUMBER
sodium ion
Na+1
11
23
11
12
10
calcium ion
Ca2+
20
10
20
20
18
sulfide
S-2
16
32
16
16
18
nitride
N3-
7
14
7
7
10