UNIT 1 & 2 Review First Quarter Exam Material. Periodic Table The Periodic Table of Elements shows...
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![Page 1: UNIT 1 & 2 Review First Quarter Exam Material. Periodic Table The Periodic Table of Elements shows all of the known elements, arranged by Increasing.](https://reader036.fdocuments.in/reader036/viewer/2022062518/56649ea25503460f94ba5a0a/html5/thumbnails/1.jpg)
UNIT 1 & 2 Review
First Quarter Exam Material
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Periodic Table
The Periodic Table of Elements shows all of the known elements, arranged by Increasing atomic number
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The Atom
The smallest particle of an Element is an Atom
To the right are the atoms in the Element Gold
http://www.chem.utoronto.ca/staff/DHIRANI/stm-np.jpg
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Atomic Models
Democritus Basic shapes to identify “atoms” No subatomic particles
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Atomic Models
Dalton Invisible and Indivisible No subatomic particles
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Atomic Models
Thomson Plum Pudding Positive substance containing negative
particles
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Atomic Models
Rutherford Protons in Nucleus Electrons around Nucleus
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Atomic Models
Bohr Protons and Neutrons in Nucleus Electrons around Nucleus in Orbits
N
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Atomic Models
Electron Cloud Protons and Neutrons in Nucleus Electrons around Nucleus in a cloud
formed my probability
N
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Subatomic Particles
Particle Charge Mass Location
Proton + 1 1 amu nucleus
Neutron 0 1 amu nucleus
Electron - 1 0 Outside the nucleus
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Isotope
An Isotope is an atom with the same number of protons, but a different number of neutrons. Changing the neutrons changes the mass of the atom.
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Isotope Examples
Carbon-13 and Carbon-12The 13 and the 12 represent
different masses for each atom. The “-” is a dash, not a negative sign.
13C and12C are also ways to indicate different masses
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Protons
Atomic number = # Protons
Carbon has 6 Protons
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Electrons
Atomic number = # Electrons Unless there is a charge
Fluorine has 9 electrons F-1 has 10 electrons Sodium has 11 electrons Na+1 has 10 electrons
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Neutrons Atomic mass - # protons = # neutrons
Carbon-12 (mass)12 – (protons)6 = 6 neutrons
Carbon-13 (mass)13 – (protons)6 = 7 neutrons
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Drawing Bohr Models Protons and Neutrons in
nucleus Electrons in rings outside of
nucleus
Ring 1 = 2 electronsRing 2 = 8 electronsRing 3 = 8 electronsRing 4 = 18 electronsRing 5 = 18 electronsRing 6 = 32 electronsRing 7 = 32 electrons
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Chemical Formulas
Represents the number of each type of element bonded together in a compound
Remember to Multiply when there are parenthases
Calcium Phosphate, Ca3(PO4)2
Ca-3, P-2, O-8
13 total atoms in one molecule of the compound.
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Kinetic Theory
Kinetic Theory states that atoms and molecules are in constant Motion
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Phase Changes Point C = Boiling
from Liquid to Gas
Point B = Liquid Form
Point A = Melting from Solid to Liquid
The plateau (flat part of the graph) represents the phase change. The temperature of the substance does not rise (or fall) until all of it has changed phases
Time
Tem
pera
ture
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A
B
C
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Moles Amedeo Avagadro came up
with the “Chemist’s Dozen” 1 mole contains 6.02 x 1023
Particles
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Mole Continued
The mass of one mole of any element is the same as the molar mass. Example: 1 mole of C = 12.011 grams
This means that 6.02 x 1023 atoms of Carbon has a mass of 12.011 grams.
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Sig Figs Placeholders are NOT significant
figures. With Addition/Subtraction line up the
decimals. With Multiplication/Division the
number of sig figs is based on the number that has the least number of sig figs.
Refer to the sig fig worksheet for complete rules.
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Answers to sig fig problems Determine the number of significant figures in each
measurement. 508.0 L ________4____________ 0.008204 g_________4___________
Round all numbers to four significant figures. Write the answers to e-h in scientific notation.
847950 kg ___847900_________ 38.5421 g____38.54__________
Complete the following addition and subtraction problems. Round off the answers when necessary
43.62 + 51.0 + 8.73 = ______103.3_________ 258.3 - 257.11 =_____1.2__________
Complete the following calculations. Round off the answers to the correct number of significant figures.
24 x 3.25 = _____78__________ 120 / 10 = ________10__________
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Density
Density is a ratio of mass and volume. How tightly packed?
D = Density = Mass Volume
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Separating Mixtures
In the separating mixtures lab the four methods of separation were listed. Filtration Decanting Evaporation Distillation
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Mixtures
A Heterogeneous mixture is one where the different parts can be easily seen.
o A Homogeneous mixture is one where the particles are mixed so well that the separate parts cannot be seen.
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Saturated vs Unsaturated
Saturated: Contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure.
• Unsaturated: Contains less dissolved solute for a given temperature and pressure than a saturated solution; has further capacity to hold more solute.
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Changes
A Chemical change occurs when atoms interact and rearrange to form new substance.
A Physical change occurs when properties of the substance changes, but the identity of the substance does not change.
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Making and Breaking Bonds
When a bond is broken energy is required.
When a bond is made energy is released.