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![Page 1: A. The Atom proton neutron electron p+p+ n e–e– zero charge positive charge negative charge electrons are found in a cloud region around the nucleus.](https://reader030.fdocuments.us/reader030/viewer/2022020320/5697bf8f1a28abf838c8d494/html5/thumbnails/1.jpg)
A. The Atom
proton
neutron
electron
p+
n
e–
zero charge
positive charge
negative charge
electrons are found in a cloud region around the nucleus
nucleus contains the protons and neutrons which make up most of mass of atom
Science 10 Review
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mass number =
isotope =
# protons + # neutrons
atoms with the same # of protons but a different # of neutrons (different mass numbers)
eg) carbon-12 carbon-14
6 p+, 6 n6 p+, 8 n
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B. Periodic Table
arranged in and
group number =
period number =
groups (columns) periods (rows)
number of outer level (valence) e-
number of energy levels occupied by e-
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C. Energy Level Diagrams
atoms are which means that the
maximum number of e-: 3rd level =
2nd level =
1st level =
electrically neutral
# of p+ = # of e-
8 e-
8 e-
2 e-
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Examples
11 p+
Na
3 p+
Li
2 e-
8 e-
1 e-
2 e-
1 e-
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Your Assignment: pg 1 in workbook
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D. Ions
ions are
neutral atoms are unstable if
atoms will strive to satisfy the in order to become stable…in other words, they strive to have
particles or groups of particles that have a net charge (either positive or negative)
their valence level is not full
octet rule a full valence level and do so by giving away or taking e-
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metals give away e- and become positive ions
eg) Na+, Ca2+, Fe3+
take e- and become negative ions non-metals
eg) Cl-, P3-, O2-
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Examples
11 p+
Na
2 e-
8 e-
1 e-
2 e-
8 e-
11 p+
Na+
sodium atom sodium ion
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17 p+
Cl
2 e-
8 e-
7 e-
2 e-
8 e-
17 p+
Cl–
chlorine atom chloride ion
8 e-
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Your Assignment: 1. Draw argon and neon and compare to Na+ and Cl–
2. pgs 2,3 in workbook
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E. Elements
metals exist as
nonmetals and hydrogen
single atoms
eg) Li(s), Cu(s), Hg(l)
do not exist as single atoms – flagpole! (SHPON)
eg) H2(g), O2(g), P4(s), S8(s)
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Try These:
1. Cu(s) =
2. O2(g) =
3. Al(s) =
4. fluorine gas =
5. barium =
6. nitrogen gas =
copper
oxygen gas
aluminum
F2(g)
Ba(s)
N2(g)
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F. Ionic Compounds
eg) K+, Be2+ or metals
eg) Fe3+, Fe2+
monovalent multivalent
charges on the ions are the result of taking or giving e-
to go from formula to name: name of first ion, then brackets for charge if multivalent, then name for second ion eg) AlCl3 =
CuSO45H2O =
aluminum chloride copper (II) sulphate pentahydrate
metals + nonmetals or polyatomic ions
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Try These:
1. NiF3 =
2. MnO2 =
3. Na3PO410H2O =
4. Zn3P2 =
5. Cr2S3 =
6. MgCl26H2O =
nickel (III) fluoride
manganese (IV) oxide
sodium phosphate decahydrate
zinc phosphide
chromium (III) sulphide
magnesium chloride hexahydrate
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to go from name to formula: write the symbol for each ion, then add subscripts to balance charges
eg) calcium sulphide = iron (III) oxide =
CaS Fe2O3
Try These:
1. sodium phosphate =
2. vanadium (IV) sulphide dihydrate =
3. magnesium nitride =
4. ammonium sulphate =
Na3PO4
VS22H2O
Mg3N2
(NH4)2SO4
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Your Assignment: pgs 4,5 in workbook
***pg 4 #18 cupric = Cu2+
pg 5 #24 –3- water = trihydrate
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G. Molecular Compounds
nonmetals only
e- are shared therefore no ions are formed
no charges involved
use prefixes in naming
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eg) N2O =
CO2 =
P4O10 =
dinitrogen monoxide carbon dioxide
to go from formula to name: name of first element (including prefix if necessary), then name for second element with “ide” ending (including prefix)
tetraphosphorus decaoxide
to go from name to formula: write the symbol for each element, then use the prefixes to determine the subscripts
eg) carbon monoxide = carbon tetrachloride =
CO CCl4
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H. Acids
always have as the state and always have
Rules
1. hydrogen becomes acid
2. hydrogen becomes acid
3. hydrogen becomes acid
aqueous (aq)hydrogen
_________ide hydro_______ic
_________ate __________ic
_________ite __________ous
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Try These:
1. hydrogen iodide =
2. hydrogen phosphate =
3. hydrogen nitrite =
4. hydrogen sulphite =
hydroiodic acid
phosphoric acid
nitrous acid
sulphurous acid
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Your Assignment: pgs 6,7 in workbook
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I. States
acids –
elements –
molecular compounds –
ionic compounds –
always (aq)
can be (s), (l) or (g)…see periodic table
can be (s), (l), or (g)
either (s) or (aq)…look up on the solubility chart
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Try These:
1. NaCH3COO( ) 6. CaCO3( )
2. BaSO4( ) 7. FeSO4( )
3. KOH( ) 8. (NH4)2S( )
4. Pb(NO3)4( ) 9. Pb(SO4)2( )
5. Hg(CH3COO)2( ) 10. Ca3(PO4)2( )
aq
s
aq
aq
aq
s
aq
aq
aq
s
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J. Chemical Reactions
vs.
reaction types:
endothermic exothermic
1. hydrocarbon combustion
2. simple composition
C?H? + O2(g) CO2(g) + H2O(g)
eg) CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)
element + element compound
eg) 2 Mg(s) + O2(g) 2 MgO(s)
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5. double replacement
4. single replacement
3. simple decomposition
compound element + element
eg) 2 H2O(l) 2 H2(g) + O2(g)
element + compound element + compound
eg) Cu(s) + 2 AgNO3(aq) 2 Ag(s) + Cu(NO3)2(aq)
compound + compound compound + compound
eg) Pb(NO3)2(aq) + 2 KI(aq) 2 KNO3(aq) + PbI2(s)
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Your Assignment: pgs 9-10
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law of conservation of matter says that
we must chemical equations to conserve matter
matter cannot be created or destroyed, it can only change forms
balance
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Your Assignment: pgs 9-10 - balancing
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Your Assignment: 1. pg 10 #1, 2, 11, 13, 14 – predicting, states, balancing, reaction type
2. pg 11
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K. Significant Digits
any digit from is significant
are significant eg)
are significant eg)
are not significant eg)
1-9
trailing zeros
counted objects and constants are not included in sig digs
“sandwich” zeros
leading zeros
6.3800, 12 000
2.04, 1005.002
0.0065
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/ :
+/ :
multiply or divide then round answer to the lowest number of sig digs
add or subtract then round answer to the lowest number of decimal places
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Your Assignment: pgs 12,13 in workbook
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L. The Mole
it is a = number 6.02 x 1023 “items”
1. Molar Mass sum of the
eg) CO2 =
Al(OH)3 =
Cu(ClO3)2 =
44.01 g/mol78.01 g/mol
230.45 g/mol
individual atomic masses for each element in a compound
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2. Mole/Mass Calculations
n = m M
where: n =
m =
M =
number of moles in mol
mass in g
molar mass in g/mol
m = nM
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Example 1
How many moles are in 8.06 g of magnesium oxide?
m = 8.06 gM = 40.31 g/moln = ?
n = m M = 8.06 g 40.31 g/mol = 0.1999503 mol = 0.200 mol
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Example 2
What is the mass of 0.677 mol of potassium sulphide?
n = 0.677 molM = 110.27 g/molm = ?
m = nM = (0.677 mol)(110.27 g/mol) = 74.65…g = 74.7 g
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Your Assignment: pgs 14,15 in workbook