Semester 1 Final
Whiteboard Review!
Identify the following data as being
qualitative or quantitative:
a.
b.
c.
d.
qualitative
Blue and fuzzy________________
1.045 m _________________
quantitative
qualitative
warm and dry _______________
quantitative
101°F _____________________
Identify the standard SI units for the following
quantities:
mole
a. amount of substance _____________
meter
b. length _______________________
second
c. time _______________________________
d. mass ______________________
kilogram
m3 also cm3 and mL
e. volume _____________
f. density ______________________
kg/m3 or g/cm3 or g/mL
Identify the following measurements as being
accurate, precise, both, or neither:
a. The actual mass is 6 g and the experimental
measurements are 3.01g, 2.99g, 3.00g precise
b. The actual length is 4.50cm and the experimental
measurements are 4.49cm, 4.51cm, 4.48cm both
c. The actual temperature is 23°C and the neither
experimental measurements are 32°C, 18°C, 37°C
How many significant figures are in each of
the following measurements?
3
a. 28.6g ______________
3
b. 3440 cm ____________
c. 3440. cm ____________
4
d. 0.004604 L___________
4
5
e. 0.0067000 kg__________
7
f. 150.0000m ____________
What is the equation for density?
D = M/V
A sample of Aluminum metal has a mass of
8.40g. The volume of the sample is 3.1cm3.
Calculate the density.
D = M/V = 8.40g/3.1cm3 = 2.7097g/cm3
 2.7g/cm3
The density of aluminum is 2.7 g/cm3.
You have a sample that weighs 8.4
grams. What is the volume of your
sample?
D=M
V
V = M = 8.4 g
D 2.7 g/cm3
= 3.1 cm3
What is the name for the ratios we
use to convert between one unit to
another?
Conversion factors!
Show your work to convert 5.712
kilograms to milligrams. Circle the
conversion factors you use.
5.712 kg x 1000 g x 1000 mg = 5,712,000 mg
1 kg
1g
You find 13,406,190 pennies. If each
penny weighs 4 grams, how much did
all that loot weigh (in pounds)? (2.2
Pounds = 1 Kilogram)
13406190 pennies x 4 g x 1 kg x 2.2 pounds =
1penny 1000 g 1 kg
117,974.5 pounds
What is the relationship between
frequency and wavelength for EM
radiation?
c = λν
c = wavelength * frequency
What is the frequency of light with a
wavelength of 4.257 x 10-7 cm?
c = wavelength * frequency
frequency = 3.0 x 108 m/s = 7.047 x 1016 Hz
4.257 x 10-9 m
What is the relationship between the
frequency of light and the energy it
contains?
E = hν or E = hc/λ
h = Planck’s constant 6.626x10-34 J s
Note: this is the energy of a single photon of
light of frequency ν.
If gamma radiation from cobalt-60
(used in nuclear medicine) has a
wavelenghth of 1.00 x 10-3 nm, what
is the energy of a photon of this
radiation?
E = hc/λ = 6.626x10-34 J*s x 3.00x108 m/s =
1.00 x 10-12 m
= 1.99 x 10-13 J
If gamma radiation from cobalt-60
(used in nuclear medicine) has a
wavelenghth of 1.00 x 10-3 nm, what
is the energy given off by a mole of
cobalt-60?
E = hc/λ = 6.626x10-34 J*s x 3.00x108 m/s =
1.00 x 10-12 m
x 6.022 x 1023 photons = 1.20x1011 J/mol
1 photon
1 mole
1.9878 x 10-13 J
What is the energy in joules of a
photon whose frequency is 3.55 x
1017 Hz?
E = hv = 6.626x10-34 J*s x 3.55x10171/s =
2.35 x10-16 J
How long would it take a radio wave
with a frequency of 7.25 x 105 Hz to
travel from Mars to Earth if the
distance between the two planets is
approximately 8.00 x 107 km?
8.00 x 107 km x 1000 m x 1 s = 267 seconds
1 km 3.0 x 108 m
Compare the frequency, wavelength,
energy and speed of gamma rays
and radio waves
Frequency
Gamma rays
Higher frequency
Radio waves
Lower frequency
Wavelength
Smaller wavelength Longer
wavelength
Energy
Speed
Higher energy
Same (c)
Lower energy
Same (c)
What is the formula for calculating
percent error?
%Error = actual value – experimental value
X 100%
actual value
A student measures the mass of a
sample to be 10.26 grams, but the
actual mass is 9.88 grams. What is
their percent error?
% error = (9.88 - 10.26) x 100% = -3.85%
9.88
A student measures the mass of a
sample to be 2.04 grams, but the
actual mass is 3.20 grams. What is
their percent error?
% error = (3.20 – 2.04) x 100% = 36.25%
3.20
Atoms of the same element with a
different mass are called...
Isotopes!
You have an element with a mass
number of 120 and has 70 neutrons.
What element do you have?
120 - 70 = 50 protons → Tin! (Sn)
What is the most common isotope of
Chromium? How many neutrons
does it have?
Chromium - 52, 28 neutrons
Element X has three isotopes: one
has a mass of 60.5 amu and is 78%
abundant. Another has a mass of
62.4 and is 19.5% abundant. And the
third has a mass of 64.7 and is 2.5%
abundant. What is the average
atomic mass of Element X?
60.5(0.78) + 62.4(0.195) + 64.7(0.025) = 61.0 amu
Find the molar mass of Chlorine.
35.45 g/mol
Find the molar mass of CO2
12.01 + 2(16) = 44.01 g/mol
If you have 18 grams of Beryllium,
how many moles do you have?
18 grams x 1 mole = 2 moles
9 grams
If you have 3.0 moles of carbon, how
many atoms do you have?
3 moles x 6.022 x 1023 atoms = 1.8 x 1024 atoms
1 mole
If you have 12 grams of Magnesium
how many atoms do you have?
12 g Mg x 1 mol x 6.022 x 1023 atoms= 3.0 x 1023atoms
24.31 g
1 mol
What is the molar mass of ethanol
C2H6O?
2 x 12.01 + 6 x 1.01 + 16 = 46.08 g/mol
If you have 26 grams of NaCl, how
many moles do you have?
Molar mass = 23 + 35.45 = 58.45 g/mol
26 g NaCl x 1 mol = 0.44 mol
58.45 g
This is the distance between
corresponding points on adjacent
waves.
Wavelength!
Name the branch of chemistry that
identifies the components and
composition of materials.
Analytical chemistry
Name the branch of chemistry that
uses mathematics and computers to
design and predict the properties of
new compounds.
Theoretical chemistry
Name the type of research done to
solve a problem
Applied Research
What is the smallest unit of an
element that maintains the
properties of that element?
An atom!
What is the definition of matter?
And give an example of something
that is NOT matter.
Anything that has mass and takes
up space. → Energy is not matter!
Give an example of an EXTENSIVE
PROPERTY.
Volume, mass, amount of energy,
size, etc.-- depend on the amount
of matter present
What state of matter has a definite
volume but indefinite shape?
Liquid!
Give an example of a chemical
property.
reactivity with air, water, oxygen,
etc.
Is carbon dioxide subliming (turning
from solid to gas) an example of a
physical or chemical change?
Physical change!
Give an example of a chemical
change.
Iron rusting
Coal burning
Hydrogen and oxygen combining to
make water
In the following reaction, what are
the reactants?
Fe + O2 → Fe2O3
Fe and O2
A solution is an example of what
kind of mixture?
Homogeneous mixture!
Composition is uniform throughout
the mixture
A tossed salad is an example of
what kind of mixture?
Heterogeneous mixture – the
composition of the mixture differs
throughout the mixture.
Every sample of a _________ has
exactly the same characteristics and
composition.
Pure substance
True or False: A compound is a pure
substance.
TRUE!!! An element is also a pure
substance
Vertical columns in the periodic
table are called ________.
Groups!
These elements are solid, ductile
and conduct electricity and heat
well.
Metals!
Platinum is a member of this family
of elements.
Transition metals
These elements surround the stairstep on the periodic table and have a
mix of properties between metals
and nonmetals.
Metalloids
This group of elements are the most
reactive metals on the periodic table.
Alkali metals!
What is the most reactive metal on
the periodic table?
Francium! Reactivity of metals
increases as you go down the
group.
This group of elements are the most
reactive non-metals on the periodic
table.
Halogens.
What is the most reactive nonmetal
on the periodic table?
Fluorine! Reactivity of nonmetals
increases as you go up the group.
What is the element symbol for
Mercury?
Hg
How many meters are in a
Megameter?
1,000,000 or 1 x 106
How many micrometers are in a
meter?
1,000,000 or 106
Give an example of a derived unit
Density, volume, molar mass,
energy
The following illustrates what law?
C + O → CO or C + O2 → CO2
Law of multiple proportions: If two
or more different compounds are
composed of the same two
elements, then the ratio of the
masses of the second element
combined with a certain mass of the
first element is always a ratio of
small whole numbers.
What was determined from Millikan’s
oil drop experiment?
Charge and mass of an electron
Atoms of an element have the
same...
Atomic number or # of protons
What phenomena gives evidence
that light acts as a particle?
The photoelectric effect
Draw a picture illustrating Bohr’s
model of the atom and how it relates
to flame colors and atomic spectra.
What is the name for a 3
dimensional space around the
nucleus where an electron may be
found?
Orbital!
How many orbitals are in the 4th
energy level?
16
Draw the correct orbital notation for
Phosphorus.
Write the full electron configuration
for Strontium (Sr) How many
valence electrons does it have?
1s22s22p63s23p64s23d104p65s2
2 valence electrons in the 5s
subshell (electrons in the highest
occupied energy level)!
Use the noble gas shortcut to write
the configuration for Lead. How
many valence electrons does it
have?
[Xe]6s24f145d106p2
4 valence electrons! (only count the
electrons in the highest occupied
energy level, n=6)
How many valence electrons does
Germanium have?
4 valence electrons!