chem ch 1 and 16
Download
Report
Transcript chem ch 1 and 16
Chapters 1 and 16
exothermic-
energy is released
in the rxn
exo- out
takes place
without help
endothermic-
energy is absorbed
in rxn
endo- in
have to have energy
in order to occur
the study of the composition of
substances and the changes they
undergo
energy is involved in accomplishing
these changes
all of those substances are chemicals
chemical- substance that has a definite composition
water- H2O
sucrose- C12H22O11
hematite- Fe2O3
2 major:
1. inorganic- concerns
substances that are usually
without carbon
2. organic- study of substances
containing carbon
subst from living things
1. basic research- carried
out for the sake of
increasing knowledge
chance discoveries can
occur and have
changed our lives!
2. applied researchcarried out to solve
problems
depletion of ozone layers
by CFCs led scientists to
develop new refrigerants
technological
developmentproduction and
use of products
that improve
our quality of
life
Which of the
following could
be called
matter?
anything that has a volume and a mass
mass- measure of the amount of
matter
use a balance to measure
volume- amount of space a 3D object
takes up
many forms of matter
fundamental building
blocks of matter:
atoms and molecules
What’s the difference?
atom- smallest unit of an element
that maintains the chemical
identity of that element
molecule- smallest unit of a
diatomic element or a compound
that retains all the properties of
that subst
elements generally make up
molecules
these particles make up elements and
compounds
What’s the difference?
elements- pure subst that CANNOT
be broken down into simpler, stable
subst; made of 1 kind of atom
compound- subst that can be
broken down into simpler, stable
subst
usu made from 2 or more kinds of
atoms
used to distinguish between subst
and to separate them
help to reveal unknown subst
ALL matter has many properties by
which it can be grouped
properties are either intensive or
extensive
do NOT depend on the
amount of matter
examined
same for a 0.5g sample
as 500kg sample
ex: melting point,
boiling point, density,
conduction of
electricity
DO depend on the
amount of matter
present
there will be a difference
in a 0.5g sample and a
500kg sample
ex: volume, mass,
amount of energy in
sample
properties can also be grouped into 2
general categories:
1. physical properties- characteristic
that can be observed or measured
without changing the identity of the
substance
ex: color, density, hardness, melting
point, boiling point
2. Chemical
properties- prop that matter
exhibits as it undergoes changes that
transform it into different subst
easiest to see as matter reacts to form
new subst
ex: reactivity with oxygen, flammability
1. physical chg- a
change in a subst
that does NOT
involve a chg in the
identity of the
subst
ex: melting, boiling,
grinding, tearing,
cutting
2. chemical changes-
aka chemical
reactions- a chg in
which the subst is
converted into
different subst
ex: rusting,
tarnishing, burning
some phy chg are part of an important class
of chgs called change of state
phy chg of a subst from one state to
another
4 main states of matter:
STATES OF MATTER FOLDABLE
2. chemical changes-
aka chemical
reactions- a chg in
which the subst is
converted into
different subst
ex: rusting,
tarnishing, burning
magnesium plus oxygen yields magnesium oxide
Mg + O2 MgO
parts of chem rxn:
1. reactants- the substances that react in the
chem rxn
arrow points AWAY FROM reactants
products- the subst that are
formed by the chem chg
arrow ALWAYS POINTS TO
products
3. arrow stands for yields
2.
ex: p. 10 fig.7
ALL changes (physical OR chemical) will
involve energy
can be different forms, like heat and light
boundaries between phy and chem chgs are
not always very clear
in any chg, the total amount of energy
involved DOES NOT change
the Law of conservation of energy
tremendous variety of forms of matter
can be categorized into 2 groups:
1. pure substance- composition is same
thruout
can be elements or compounds
2. mixture- contains more than 1 subst;
can vary in composition and
properties
every sample has a fixed composition
H2O (by mass, 88.8% O and 11.2% H)
every sample has exactly the same
characteristic properties
properties can be used to identify the
subst
either elements or compounds
blend of 2 or more kinds of matter, each
retaining its own identity and properties
usu physically combined and can be
separated
properties of mixture are a combination of
the properties of subst that make it up
2 types of mixtures:
homo- same
looks the same
thru-out
uniform in
composition
aka- solutions
may be solids,
liquids, gases
solvent- part that does
the dissolving
usu water
aka- the universal solvent
1.
2. solute- part that is
dissolved
hetero- different
may look different
composed of
more than one
phase
separated by
boundaries called
interfaces
substances composed of only one kind of atom
ALWAYS have the same composition
ex: gold, mercury, hydrogen
substances composed of more
than one kind of atom always
arranged in definite ratios
ex: copper II sulfate, CuSO4
sucrose, C12H22O11
one or more subst are used
up
1 or more new subst are
formed
energy is absorbed or
released
color change
formation of precipitate (ppt)
gas bubbling
energy changes- heat, light
exothermic- energy is
released in the rxn
exo- out
tend to take place
without help
endothermic rxn- energy is absorbed in
the rxn
endo- inside
have to have input of energy to occur
occur with NO changes
in the composition
can be:
chgs of state
cutting/breaking
dissolving
distillation
fractional
crystallization
phy and chem chgs (
) always
accompanied by energy changes
energy changes occur betw sys and
surroundings
energy transfer as a result of temp
difference is HEAT
can measure energy chg using units called
Joules (J)
older unit used is calorie
1 cal = 4.184 J
food calorie is a larger unit
1 CAL = 1 000 cal
convert betw units
study of the transfer of heat energy that
accompany chem rxns and physical chg
temp- is a measure of the average kinetic
energy of the particles in a sample of matter
greater KE, higher temp, hotter it feels
K= oC + 273
HEAT- measure of the total amount of kinetic
energy of the particles in a sample of matter
ALWAYS moves from matter at a higher temp
to matter at a lower temp
fig 1, p.532
calorimeter- device
used to measure the
energy given off
during chem and
phy chgs
Will you take a
piece of the crust
with your finger?
Will you stick your
finger into the
filling of the pie?
Why won’t you?
Is there a
difference?
some materials tend to heat up and
stay hotter longer than other materials
dependent on obj’s SPECIFIC HEAT
amount of energy required to raise
the temp of 1 g of a subst by 1oC (or
1K)
Cp
units are: J/(goC)
Cp H2O= 4.184J/goC
table 1, p.533
use the formula:
q
= m x Cp
x Temp
heat = mass x specific heat x (Tf-Ti)
when heat is gained, Tf-Ti
when heat is lost, Ti-Tf
ex: How much heat energy is needed to increase the temp
of 755g of Fe from 283oC to 403oC?
How much energy must a refrigerator absorb from 225g of
water so that the temp of the water will drop from
35.5oC to 5.0oC?
What mass of water is required to absorb 470 000J of
energy from a car engine while the temp increases from
25.0oC to 82.5oC?
Apiece of copper alloy with a mass of 85.0g is heated from
30.0oC to 45.5oC. In the process, it absorbs 523J of heat.
What is its specific heat?
ex: How much heat energy is needed to increase the
temp of 755g of Fe from 283oC to 403oC?
How much energy must a refrigerator absorb from 225g
of water so that the temp of the water will drop from
35.5oC to 5.0oC?
What mass of water is required to absorb 470 000J of
energy from a car engine while the temp increases
from 25.0oC to 82.5oC?
Apiece of copper alloy with a mass of 85.0g is heated
from 30.0oC to 45.5oC. In the process, it absorbs 523J of
heat. What is its specific heat?
any heat lost by 1 quantity of matter must
be gained by the other quantity of matter
in a system
one will lose heat to the other until both
are at the same temp
(law of conservation of energy)
fig 1, p.532
If a piece of gold with amass of 45.5g and a temp of
80.5oC is dropped into 192g of water at a temp of 15.0oC,
what is the final temp of the system?