Transcript CHEMISTRY SOL REVIEW

CHEMISTRY SOL REVIEW
SOL 2
UNIT 2 - Matter
Matter is anything with mass & _______
 Volume
 ____ substances are types of matter with
definite & uniform characteristics.
 Pure
 For example, _____ contain only one
kind of atom.
 Elements
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UNIT 2 - Matter
A _____ is another pure substance that
is made of more than one type of atom &
can only be broken down by chemical
means.
 Compound
 _______ are types of matter with 2 or
more substances that can vary in
composition & properties
 Mixtures
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UNIT 2 - Matter
A _______ mixture has a uniform
composition (Stainless steel, KoolAid)
 Homogeneous
 _____ is considered the universal solvent
 Water
 The particles dissolved in a solvent are
called the __________
 Solutes
 A _____ is really a heterogenous mixture
but LOOKS like a solution (milk)
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UNIT 2 - Matter
Phase changes are _____ changes (physical
or chemical)
 Physical
 The process of a solid becoming a gas
(without becoming a liquid first) is ___
 Sublimation
 What state of matter has the strongest IMF?
 Solid
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UNIT 2 - Matter
Name the 4 things used as evidence of a
chemical reaction occurring
 Production of a gas (odor or bubbles)
 Color change
 Release/absorption of energy (light or heat)
 Forming a precipitate (chunks )
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UNIT 3 – History of the Atom
5 part atomic theory – all matter made of
atoms
 Dalton
 Cathode Ray Tube experiments, Plum
Pudding model, Electrons have mass & a
negative charge
 JJ Thomson
 Measured charge of an electron
 Millikan
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UNIT 3 – History of the Atom
Passed alpha particles through gold foil
and found that the nucleus is dense and
positively charged
 Rutherford
 Electrons found in levels or shells around
the nucleus
 Bohr
 Electrons behave like waves (ceiling fan)
 de Broglie
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UNIT 3 – History of the Atom
Atomic number gives us # of ____ in an
atom of each element
 Protons
 Mass number is calculated by adding __
 Protons plus neutrons
 Different isotopes have different #s of __
 Neutrons
 Different __ have different #s of electrons
 Ions
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UNIT 3 – History of the Atom
Calculate the average atomic mass of
copper if copper has 2 isotopes. 69.1%
has a mass of 62.93 amu and the rest has
a mass of 64.93 amu.
 (.691 * 62.93) + (.309 * 64.93)
 63.55
 Flourine – 19 has how many neutrons?
 10
 What is the molar mass of carbon?
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UNIT 3 – History of the Atom
You find an artifact with a C-14:C-12 ratio
that is 1/16 the modern ratio. The half life
of C-14 is 5715 years. How old is the
artifact?
 22860 years
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UNIT 4 – Electron Configuration
What is the longhand electron configuration
for N?
 1s2 2s2 2p3
 For Fe?
 1s2 2s2 2p6 3s2 3p6 4s2 3d6
 What is the shorthand config for Ca?
 [Ar] 4s2
 The electrons in the outermost shell are
called the _______ electrons
 Valence
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UNIT 4 – Electron Configuration
How many p orbitals are there?
3
 What shape is a p orbital?
 Bowtie or dumbbell
 How many electrons can be held in d
orbitals?
 10
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UNIT 4 – Electron Configuration
How many valence electrons does oxygen
have?
6
 The rows in the periodic table are called
 Periods
 Draw a Lewis dot diagram for Nitrogen
 When an electron returns to its ground
state after being excited, it releases energy
and emits a _____, or a particle of light.
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Unit 5 – The Periodic Table
The elements on the right side of the
staircase are _____
 Nonmetals
 The first column or group of elements
are called the ____
 Alkali metals
 Group 7 is called the ___
 Halogens
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UNIT 5 – The Periodic Table
The d-group elements are called the __
 Transitional metals
 The f-block elements are called the ___
 Inner transition metals
 What happens to atomic radius as you
move from top to bottom down the
periodic table?
 Gets bigger
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UNIT 5 – The Periodic Table
The energy required to remove an
electron from an atom is called __
 Ionization energy
 What happens to ionization energy as you
move from left to right across a period?
 Gets bigger
 An atoms affinity for electrons in a
compound is called its ___
 Electronegativity
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ANNOYING 2009 Question
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Potassium (K) has a smaller atomic mass than (Ar)
even though the atomic number of potassium is larger
than the atomic number of argon. Which of the
following BEST accounts for this observation?
F At STP, K is in the solid phase, but argon is gas
G It is easier for a potassium atom to lose an
electron than it is for an argon atom
H The most common isotopes of argon have more
protons than the most common isotopes of potassium
J The most common isotopes of potassium have
fewer neutrons than the most common isotopes of Ar