video 1
.1
mass,
volum
e,
densit
y
what is chemistry?
!
!
!
Qualitative Measurements: descriptive,
non-numerical ________________
Quantitative Measurements: are in the
form of _____________ and UNITS
What is matter?
!
matter can be described with:
!
The study of ___________ and the
changes it undergoes…
Matter is anything that has ________ and
takes up _______________.
Qquantitative calculations
!
!
Mass: the amount of __________ an
object contains (this is different than
weight, which is mass plus gravity).
Volume: The amount of ___________ a
substance occupies.
1
how do we measure mass?
!
how do we measure volume?
Quadruple Beam Balance
!
V = l x w x h (regular solid)
!
!
Electronic Balance
!
ex. V = _________ cm3
Graduated Cylinder (liquids)
Read bottom of MENISCUS
!  ex. V = ___________ mL
!
!
Units: grams (g)
measuring volume: irregular solids
!
Water displacement
method
1. Measure the initial
volume
!  2. Measure final
volume with object
!  3. The difference
(subtract) is the
volume of the object
!  ex. ________________
!
stop and think
!
What is the volume of the solid?
a. 69 mL
b. 65 mL
!  c. 4 mL
!  d. 58 mL
!
!
2
density
Ratio of mass of an object to its volume
!  Use density formula:
!  Located on Table T
!
example 1
!
stop and think
!
What is the density of an object with a
mass of 57.8 g and a volume of 112.4 mL?
What is the density of an object with a
mass of 60 g and a volume of 2 cm3?
example 2
!
An object has a volume of 825 cm3 and a
density of 13.6 g/cm3. Find its mass.
3
stop and think
!
What is the mass of an object with a
density of 0.3456 g/cm3 and a volume of
112.4 cm3?
what to do if density isn’t given
If asked to solve for mass or volume, but
density isn’t given: USE Table S
!  Example: The volume of an aluminum
sample is 251 cm3. What is the mass of
the sample?
!
!
Look up the density of aluminum on Table S:
2.70 g/cm3
stop and think
!
Determine the mass of a silver object with
a volume of 82 cm3?
4
video 1
.2
t e m pe
r
conver ature
sions
and
percen
t erro
r
what is temperature?
!
temperature scales
Temperature: a measurement of average
____________ energy. (Temperature is
NOT the same thing as __________)
celsius scale
Freezing point of water: _____°C
!  Boiling point of water: ______°C
!  Below zero is NEGATIVE
!
1
kelvin scale
Freezing point of water: ________ K
!  Boiling point of water: ________ K
!  Theoretical point of _____________ is
when all molecular motion stops
!  No negative numbers
!  Divisions (degrees) are the same as in
Celsius
!
converting between
temperature scales
!
Formula: K = °C + 273
!
Located on Table T
stop and think
!
If the temperature of a substance was
raised 50°C, how many Kelvin was it
raised?
example 1
!
What is the temperature in Kelvin of an
object that is 55°C?
2
example 2
!
What is the temperature in Celsius of an
object that is 150K?
stop and think
!
What is the temperature in Celsius of a
liquid that is 656K?
accuracy vs. precision
Accuracy: how close a measurement is to
the ___________ or true value
!  Precision: how close a series of
measurements are to ______________
!
percent error
!
Measurement of _______________
!
the % that the measured value is “off” from
the accepted value
Measured value: value you “get”
!  Accepted value: value you “should get”
!  Formula found in Table T:
!
3
example 1
!
A student determines the density of a
substance to be 1.40 g/mL. Find the
percent error if the accepted value of the
density is 1.36 g/mL.
stop and think
!
What is the percent error if a student
measures an object to be 56.2 cm and the
actual length is 56.9 cm?
stop and think
!
In a lab experiment, you are told by your
teacher that the actual amount of sugar in
a can of Coke is 39 g. You experimentally
determine it to be 37 g based on your own
data and calculations. What is your
percent error?
4
video 1
.3
precis
ion and
signif
icant f
igures
significant figures (sig figs)
Indicate _____________ of a measurement.
!  Recording Sig Figs
!
!
Sig figs in a measurement include the known
digits plus a final estimated digit (precision
of instrument)
______ cm
example measuring length:
Device is marked to the ones place, so estimate the tenths place: ___________
We know for sure that the object is more
than 2 but less than 3.
!  We know for sure that the object is more
than 2.7 but less than 2.8
!  This ruler allows us to estimate the length
to ___________cm.
!
Device is marked to the tenths place, so estimate the hundreths place: _______
Device is marked to the hundreths place, so estimate the thousandths place: ____
Device is marked to the tens place, so estimate the ones place: _________
Device is marked to the hundreds place, so estimate the tens place: ________
1
stop and think
!
What is the length of the red line?
stop and think
!
What is the length of the red line?
stop and think
!
What is the volume of the liquid?
2
video 1
.4
counti
ng sig
figs
rules for counting sig figs
!
If a decimal is _________, start on the
Atlantic side (right) with the 1st non-zero
number & count every number after that.
P
!
!
If a decimal is Absent, start on the Atlantic
side (right) with the 1st non-zero number &
count every number after that.
5400 = ____ sig figs
!  5401 = ____ sig figs
!  100 = ____ sig fig
!
!
A
If a decimal is _________, start on the
Pacific side (left) with the 1st non-zero
number & count every number after that.
If a decimal is Present, start on the
Pacific side (left) with the 1st non-zero
number & count every number after that.
2545.300 = ____ sig figs
!  0.00453 = ____ sig figs
!  0.07001 = ____ sig figs
!
1
stop and think
!
How many sig figs in 23.500 m?
stop and think
!
How many sig figs in 53,000 km?
stop and think
!
How many sig figs in 0.0800 g?
2
video 1
.5
roundi
ng sig
figs
in calc
ulatio
ns
rules for calculating with sig
figs
Multiplying/Dividing: round answer to the
fewest number of ____________.
!  Ex. (13.91g/mL)(23.3mL) = 324.103 g
!
4 SF
3 SF
what do Ii round my answer to?
!
Every measurement has some error in it.
When performing calculations, an answer
can never be more _________ than your
least precise measurement.
stop and think
!
Round answer to the proper # of sig figs.
!
15.30g / 6.4mL =
Round to
______ SF
____ g
1
stop and think
!
Round answer to the proper # of sig figs.
!
rules for calculating with sig
figs
!
18.9mL x 0.84g/mL =
!
Adding/Subtracting: round to the fewest
number of _________________.
Ex. 3.75 mL + 4.1 mL = 7.85 mL
2 Decimal
Places
1 Decimal
Place
Round to ____
Decimal Place
___ mL
stop and think
!
Round answer to the proper # of sig figs.
!
28.9g – 0.85g =
stop and think
!
Round answer to the proper # of sig figs.
!
80.4 mm – 16.532 mm =
2
video 1
scient .6
ific
notat
ion
scientific notation
A way to represent very
_________________numbers conveniently.
!  For example:
!
The mass of a hydrogen atom is
0.00000000000000000000000167g.
!  2 g of H2 contains
602,000,000,000,000,000,000,000 molecules.
!
scientific notation
!
Scientific notation is written as:
The product of two numbers: a coefficient and a
10 raised to a power.
!  The coefficient (number written first) is always
a number between _____________.
!  Example:
!
converting to scientific
notation
1. For #’s greater than 1, move decimal to
the _________ until you get to a number
between 1 and 10. The number of places
moved = _____________ number.
!  Ex. 45,450 g =
!
!  1.67
x 10-24 g
!  6.02 x 1023
1
converting to scientific
notation
stop and think
!
2. For #’s less than 1, move decimal to the
__________ until you get to a number
between 1 and 10. The number of places
moved = ____________ exponent number.
!  Ex. 0.00453 mL =
Convert the following to scientific notation:
!
stop and think
!
Convert the following to scientific notation:
!
0.00009 cm =
!
45,700 m =
converting from scientific
notation to standard notation
Move the decimal place the number of times
indicated by the exponent.
!  To the ________ if the exponent is positive.
!  To the _______ if the exponent is negative.
!  Example: 4.5 x 10-2 =
!
2
stop and think
!
Convert the following to standard notation:
!
stop and think
!
9.6 x 103 =
!
calculating with sci notation
using a calculator
Ex. (5.44 x 107 g)/(8.10 x 104 mol) =
!  Type on your calculator:
5.44 EXP 7 ÷ 8.10 EXP 4 ENTER
!
EE
Convert the following to standard notation:
1.2 x 10-4 =
stop and think
!
3.95 x 102/1.5 x 106 =
EE
= 671.60493 = 672 = 6.72 x 102 g/mol
3
stop and think
!
3.5 x 102 x 6.45 x 1010 =
4
video 1
.7
metri
conver c
sions
quantitative measurements
The Metric System (SI): System of
measurement used in _________ and in
most countries
!  The BASE UNITS of measurements: Found
in Reference Table D
!
table d - base units
prefixes
Used to modify base units of
measurements (Found on Table C)
!  Example: gram (g)
!
1
stop and think
!
What is a base unit?
a. cg
!  b. g
!  c. mg
!  d. kg
!
converting units using table c
1. Find the difference between the
_________ of the two prefixes on Table C.
!  2. Move the decimal that many places.
!
Move the decimal _______ when going from a
smaller prefix to a larger prefix.
!  Move the decimal _______ when going from a
larger prefix to a smaller prefix
!
where are the base units?
!
Table C
example 1
!
Convert 5.2 cm = ________ mm
•  The difference
between the two
factors (-2 and -3) is 1
•  Since you are moving
from a larger to a
smaller prefix, you
move the decimal one
place to the right.
Base units (grams, meters, liters, etc.) fit in at arrows.
The factor would be 100
2
example 2
!
Convert 45.5 mm = ________ m
stop and think
!
Convert 20 cm = ________ m
•  The difference
between the two
factors (-3 and 0) is 3
•  Since you are moving
from a smaller to
larger prefix, you
move the decimal
three places to the
left.
stop and think
!
Convert 0.0032 L = ________ mL
stop and think
!
Convert 45
m = ________ nm
3