Download Metric Unit – Chapter 1

Name ________________________________________
Periods 1 & 6
Final Review
Unit 1 The Metric Unit:
Chemistry – study of the ______________________________________, and the
__________________________________________________________________
Chemistry is the science that __________________________________________
______________________________________________________________ and
engages in the synthesis and analysis of _________________________________.
--Webster’s
***OR chemistry is ______________________________________________***
Matter – anything that _________________________________________
___________________________________________________________
OR ________________________________________________________
____________________________________________________________
Scientific Notation … making #s __________________.
Scientific notation provides an easy way to represent #s that are really really
_______________ and really really ___________________
Scientific notation = a ___________________ # in ones place (in front of the
decimal) with nothing to the left of it __ . __ __ __ __...
↕
nonzero
400
4.1
33.1
7
0.77
To put numbers into scientific notation:
________________________________________ until there is one nonzero in the
ones place with nothing to the left of it.
The Final Review – Periods 1 & 6
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EXAMPLES:
Convert the following #s into sci. not.
7010 = ___________________
0.041 = ___________________
7.4 = ___________________
Take the following #s out of sci. not.
1.1 * 10-2 = ___________________
7 * 101 = ___________________
2.2 * 103 = ___________________
Unit 2 Matter and Energy:
Matter - _________________________________________________________________
________________________________________________________ … EVERYTHING
Matter must have: _________________ and __________________
A. Properties of Matter:
•
When you look at a particular sample of matter, you observe its ______________.
•
We classify different types of matter according to _________________________.
Physical – observed without changing the chemical _________________.
Examples: __________________________________________
Chemical – requires a change in chemical _________________ to be
observed – relates to a substances ability to undergo change.
Examples: _________________________________________
Qualitative – no observed _____________________ – no #
Examples: ________________________________________
Quantitative – includes a numeric measurement
Examples: _______________________________________
The Final Review – Periods 1 & 6
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Example: My three pennies had a volume of 1.02 ml.
Physical or chemical? Qualitative or quantitative?
Mass - ____________________________________________________________
Different from weight? ______________________________________________
B. Classifications of Matter:
Matter
Mixtures
(more than 1 ____________________)
Pure Substance
(always the same – same
_________________________
________________________)
Homogeneous
(the same
throughout)
- air =
solutions
Heterogeneous
(physically
__________________,
not the same
throughout)
- pizza
element
compound
(2 or more
_____________________
chemically bonded together)
–
A mixture = a _________________________ of two or more components.
–
Another name for a homogeneous mixture is a solution.
 Separating the components of a mixture:
Differences in ________________________ can be used to separate mixtures.

Filtration = the process that ______________________________________ in
a heterogeneous mixture is called

Distillation = the process of ________________________________________
________________________________________________________ - during
a distillation, a liquid is boiled to produce a vapor that is then condensed into a
pure liquid.
Which physical property does filtration rely on? ________________________
Which does distillation rely on? ______________________________________
The Final Review – Periods 1 & 6
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–
Distinguishing Elements and Compounds:
Element = the ___________________________________________________
_______________________________________________________________
 Oxygen and hydrogen are 2 of the more than 100 known elements.
Compound = a substance that contains _______________________________
_____________________________________________ in a fixed proportion.
 Physical methods that are used to separate mixtures cannot be used to
break a compound into simpler substances.
 To break a compound apart, you must apply _________ (usually heat /
electricity)
***The properties of compounds are totally different than the properties of the
elements they are made of.
C. States of Matter:
o Solids – rigid with a _________________________________________________
o Liquid – flowing with a ______________________________________________
o Gas – flowing, compressible – NO definite shape or volume
D. Changes in Matter:
Lab vocab.
A. precipitate – _____________________________________________________
B. exothermic reaction – _____________________________________________
C. endothermic reaction – ____________________________________________
The Final Review – Periods 1 & 6
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Physical Change – change without change in the ____________________ of the
substance – easily reversible.
- Are changes of state physical changes? ___________________________
3 states of matter:
-liquid
-solid
-gas
Chemical Change – one or more substances are converted into different (new)
substances – cannot go back without another reaction
- burning
- breaking apart a compound
- rusting
Law of Conservation of Matter / Law of Conservation of Mass: ____________________
________________________________________________________________________
Unit 3 Atomic:
Before we start (review):
__________(_)
Nucleus
ATOM
___________(_)
___________(_)
The Final Review – Periods 1 & 6
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I. Atomic Theory (1800s):
 Make sure you know that Modern Atomic Theory as described below!!!
Dalton’s Atomic Theory (1800s):
Modern Atomic Theory:
1. All matter is _________________
1. All matter is composed of
extremely small particles
called atoms.
___________________________
___________________________.
2. Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties.
3. Atoms cannot be subdivided,
created, or destroyed.
2. A GIVEN ELEMENT CAN
HAVE ATOMS WITH
DIFFERENT _____________.
3. ATOMS ARE _____________
INTO EVEN SMALLER
PARTICLES.
4. Atoms of different elements
combine in simple wholenumbered ratios to form
chemical compounds.
4. Atoms of different elements
combine in simple wholenumbered ratios to form
5. In chemical reactions, atoms
___________________________.
are _____________________
5. In chemical reactions, atoms are
_______________________.
___________________________
___________________________.
- 1897 J. J. Thomson:
- Studied ________________________ _______________.
- All metals create _____________________________________.
- Cathode ray particles are ___________________ and
____________________ _______________________.
- Thomson coined the ________________________ as another name for
_____________________ ______________ _____________________.
- Thomson’s view of the atom = _______________ _________________
with separate parts, negative ____________________ and positive
____________________________
The Final Review – Periods 1 & 6
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Representing nuclear decay and other nuclear reactions:
____________________
4
→ 234
92
90 Th + 2He
238U
_____________________
Mass # = protons + neutrons
Atomic # = protons – find this on the _______________________________
Write the nuclear symbol for Carbon with 6 neutrons _____
Write the nuclear symbol for Carbon with 8 neutrons _____
- 1909-1910 Rutherford:
- Gold foil experiments = _______________________________________
____________________________________________________________
- Atom’s appearance:
- _____________________________
- ______________________________________________
- ___________________________________________
- 1912-1913 Bohr:
- modified __________________________ model
- Electrons are located in
____________________________________________.
- Used this model to explain ________________ _________________
… ring model
-When an electron becomes excited (____________ ___________) it can
jump up to a new energy level. When it falls back down to its
_______________________ ______________ (original energy level) it
emits energy (light).
The Final Review – Periods 1 & 6
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-1919 Rutherford:
- discovered _________________________
- Carry a _______________ charge and are found in the ________.
- The number of ___________ is the atom’s ___________
____________.
- 1926 Bohr:
- Neils Bohr’s ____________________model of the atom
- ___________________________________________________
- ___________________ is dense center with _____________
_______________
- ______________________ found in specific energy levels
- 1932 Chadwick:
- discovered ___________________ - no charge, located in the
______________
- What are protons, neutrons, and electrons made of? _______________________
Vocabulary:
Isotopes - _______________________________________________________________
________________________________________________________________________
Ion - ___________________________________________________________________
________________________________________________________________________
The Final Review – Periods 1 & 6
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Fundamental parts of atoms
COMPONENT
CHARGE
electron
______
________
+1
neutron
0
APPROXIMATE
MASS (in amu)
LOCATION
IN ATOM
0.00055
shells
1.0
nucleus
_________
1.00055
• X = __________ __________
• A = __________ __________
• Z = _________ ____________
• C = ___________________
A
Z
C
X
# of neutrons = ________________________
# of electrons = ________________________
What forces act in the atom?
- ________________________________ force holds _______________ together
- _________________________________ force causes __________________
- Natural radioactivity, radioactive decay, or nuclear disintegration is the
_________________________________ of __________________ from an
element due to instability of the ___________________.
- Problems in nuclear stability occur when there are too few or too many
____________.
- All elements with an atomic number greater than _______ are radioactive.
The Final Review – Periods 1 & 6
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