final review 2013
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Final Review 2013. Chapts 1-2. - PowerPoint PPT PresentationTRANSCRIPT
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Final Review 2013
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Chapts 1-2
1. a)Hypothesis: tentative answer to a questionb) Control : used for comparisonc)Theory: explanation supported by many experimentsd)Law: relationship in nature supported by experimentse) Independent Variable: one changed by the experimenterf) Dependent variable: one changed because of the independent variable
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Review
2a) Safety: -goggles -apron -closed toe shoes -hair tied back
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Review
b) -follow directions -report accidents to teacher -place waste in designated containers -know the location of safety equipment -no horseplay
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Review
c) Flush with water for 5 minutes
d) Rinse in safety shower (fully clothed)
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Review
3. mass- electronic balance volume- graduated cylinder length – metric ruler time- stop watch temperature – thermometer
All measurements should have a NUMBER and UNIT!
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SI Units for Measurements
a) Mass – gramsb) Volume – litersc) Length – meterd) Time – secondse) Temperature - ˚C
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Accuracy & Precision
Accurate- measurements are CLOSE to the accepted value
Not accurate- measurements are NOT CLOSE to the accepted value
PRECISE – series of measurements close to each other
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Reviewc) Percent error:
d) density:
e) quantitative data: numerical data (numbers)f) qualitative data: information describing color, odor, shape etc
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Trial Group A Group B Group C
1 1.54 1.40 1.702 1.60 1.68 1.693 1.57 1.45 1.71Average 1.57 1.51 1.70
Accepted value is 1.59 g/ml
5a) Group A most accurateb) Group C precisec) None
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% error for Group ATrial Group A Group B Group C
1 1.54 1.40 1.702 1.60 1.68 1.693 1.57 1.45 1.71Average 1.57 1.51 1.70
(1.59 – 1.57) X 100 1.59
= 1.3%
5d)
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Scientific Notation
6a) 4.5 x 10-5 = .000045
b) 8.7 x 106 = 8700000
7a) 238,000 = 2.38 x 105
b) 0.00072 = 7.2 x 10-4
2 sig figs
2 sig figs
3 sig figs
2 sig figs
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Density
8)
9)
70mL
2100gDensity = 30g/mL
20mL
75g
Density = 3.75g/mL
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Density
10) 20/5 = 4g/mL B is the same
11) Read the BOTTOM of the meniscus
Volume is 43.0mL
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Graphs13a) Pie graph- percentages b) Bar graph- comparisons
c) line graph- shows how the dependent variable changes with a change in the independent variable
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Graphing Rules
1. Title
2. Labeled axes
3. Equal intervals
4. Use up most of the page
5. Use a key if needed
X-axis – independent variableY-axis – dependent variable
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Chapter 314) Definitions are in the textbooka) Cutting plastic - physical
b)Rotting meat- chemicalc) water evaporating- physical
d) Dissolving salt- physical
e) Bubbles formed when vinegar reacts- chemical
f) Gold conducting electricity- physical
g) Magnesium burning- chemical
15) bubbles- chemical change ex odor, heat, precipitate
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Definitions/examples
16)Element example- Au, Zn, Br etcCompound examples- NaCl N2O5 ZnBr2
17) Particles Energy Shape/vol
Solid tight low definiteLiquid loose medium def vol but
not shapeGas Very
loosehigh Indefinite
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Homo vs Hetero
18)Salt water- homo
b)clay and oil- hetero
c) sweet tea- homo d) kool-aid- homo e) vegetable soup- hetero f)chunky peanut butter- hetero
g) muddy water- hetero
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Separating Substances
19)Colors in black ink- chromatography b) salt water- evaporation c)sand and water- filtration d)iron filings and sulfur- magnetism f) two different liquids- distillation
Filtration
Distillation
Chromatography
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Types of MixturesParticlessize
Tyndalleffect
Settling?
Solution tiny none noColloid small yes noSuspension large n/a yes
Tyndall effect b is a suspension
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Atomic Theory Scientists21)USE THE TEXTBOOK – page 103 to 10422) Use the textbook for definitions23) See page 114 of the textbook24) Atomic # is number of PROTONS a) lithium atomic # 3 b) 3 protons and electrons c) sulfur – 16 Protons d) Lithium – 4 neutrons 25)silver-107 47 protons and 60 neutrons26)neutrons = mass – protons = 31 neutrons
57 Fe26
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Types of Radiation
27a) Alpha beta gamma b)
c)
4 He2
0 β-1
0 ϒ0
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Nuclear Equations
d) 226 222 Ra Rn + 88 86
ii) 14 14 C N + 6 7
4 He2
0 β-1
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Fission vs Fusion
28)
• Splitting a heavy nucleus
• Energy produced
• Fusing small nuclei• LARGE amounts of
energy produced• Occurs in the sun• Responsible for all
elements heavier than H
**Cheap source of energy with less pollution than burning coal, however, expensive to build the plant, problems with getting rid of nuclear waste etc
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Half- Life
29) Time
(minutes)Amount (g)
0 16518 82.536 41.2554 20.6272 10.3190 5.16
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Half- Life
29b)Time
(minutes)Amount (g)
0 10.01 5.02 2.50
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Half-Life application30) Using C-14 to determine the age of a fossil
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Isotopes
31) Mg-24 contributes the most to the average atomic mass of magnesium (closest to the number on the periodic table), so it is the most abundant in nature.
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Weighted Average Atomic Mass
32)
Element X is BORON
Isotope Mass (amu)
% abundance
Mass x %
X11 10.013 .198 1.9826X10 11.009 .802 8.8292
TOTAL: 10.812
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Chapter 533) Get definitions from the textbook34) s, p, d, f
b)
Various shapes- spherical, dumbbell etc
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Sublevels
c) Sub-Level
# electrons
s 2p 6d 10f 14
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Electronic Configurations
35) Li- 1s22s1 [He] 2s1
b) Ne- 1s22s22p6 [He] 2p6
c) Al- 1s22s22p63s23p1 [Ne] 3s23p1
d) Ca- 1s22s22p63s23p64s2 [Ar] 4s2
36) Si
b) F c) Na
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Valence Electrons
37) Beryllium (group 2A) - 2 valence e-
b) Nitrogen (group 5A) - 5 valence e-
c) Argon- (group 8A) 8 valence e-
d) Sulfur- (group 6A) 6 valence e-
e) Boron- (group 3A) 3 valence e-
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Flame Tests
38) Elements give of distinct colors when heated in a flame. The color of the flame is matched to the known element.
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Electron Configuration
39a) 4p1 – Gallium b) 5s2 – Strontium c) 6p6 – Radon d) 7s1 – Francium
40) Same column- similar ending config
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Concepts
a) Valence e- is the SAME as the group number
a) Cesium – 1 Nitrogen – 5 Oxygen – 6
c)
d) Period tells you the # of energy levels (rings)
e) s-block (groups 1 & 2) p-block (groups 3A-8A) d-block (transition metals) f-block (lanthanides & actinides)
Cs N O
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Periodic Trends
c) Ionization Energy decreases down the group increases across
Lowest IE – Francium Highest IE - Helium
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Periodic Trendsd) Electronegativity decreases down the group increases across
Lowest E – Francium Highest E - Fluorine
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Periodic Trendse) Metals become SMALLER when they turn into ions
Non-metals become LARGER
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Periodic Trends
f) Francium is most active metal. Fluorine most active non-metal.
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AKS 11b Trends on Element PropertiesFamily Group# #
valence charge Examples
Alkali 1A 1 +1 LiAlkaline earth 2A 2 +2 CaNitrogen grp 5A 5 -3 PCarbon grp 4A 4 +/- 4 SiOxygen grp 6A 6 -2 Shalogens 7A 7 -1 BrNoble gases 8A 8 0 KrInner trans f-block varies varies Utransition d-block varies varies FeRep elements A elements varies varies O
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AKS11b Metal/Nonmetal/Metalloida) Metals left, nonmetals right , metalloids
border the stairstep line. Stairstep line separates metals and nonmetals
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c) Metals - shiny, malleable, ductile, conduct electricity, react with acid Nonmetals - mostly gases, dull brittle, do not react with acids, nonconductorsMetalloids - have properties of BOTH metals & nonmetals
d) Metals mostly s and d block Nonmetals and metalloids mostly p block
AKS11b Metal/Nonmetal/Metalloid
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Chapter 8 - Ionic Bonding
1. a)
b)
CaCl2
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2a) Binary compounds – 2nd element gets “ide” b) Roman numerals used for transition metals that have more than one charge ex Fe2+
and Fe3+
2a) KBr - Potassium Bromide
b) CaCl2 - Calcium chloride
c) SnO2 - Tin (IV) oxide d) Cu(NO3)2 – Copper (II) nitrate
e) Sr(OH)2 – Strontium hydroxide
Chapter 8 - Ionic Bonding
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Ionic Bonding question #4
Name Compound Cation Anion Formula B or NB
Lithium Flouride Li+ F- LiF BSilver Oxide Ag+ O2- Ag2O BBarium carbonate Ba2+ (CO3)2- BaCO3 NBGold(III) sulfite Au3+ (SO3)2- Al2(SO3)3 NBCopper (II) hydroxide Cu2+ (OH)- Cu(OH)2 NB
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Ionic Bonding
5a) Na2SO4 - Sodium sulfate
b) SnO2 - Tin (IV) oxide
c) FePO4 - Iron (III) phosphate d) Ca(NO2)2 - Calcium Nitrite e) MgCO3 - Magnesium Carbonate f) Al(OH)3 - Aluminum hydroxide g) (NH4)3N - Ammonium nitride
h) AgC2H3O2 - Silver acetate i) Fe3P2 - Iron (II) phosphide
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Chapt 9 - Covalent Bonding
6)
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Covalent Bonding
7) Binary covalent compounds end in “ide”9) a) PH3 - phoshporus trihydride
b) CCl4 - Carbon tetrachloride
d) NO - Nitrogen monoxide f) As2O5 - Arsenic pentoxide
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Lewis Structures
10a) b)
c) d)
e)
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Covalent & Ionic Bonding
13 a) MgCl2 – Magnesium chloride
b) NO2 - Nitrogen dioxide c) HF - Hydrogen fluoride d) K3PO4 - Potassium phosphate e) NH4Br - Ammonium bromide
f) Cu(NO3)2 – Copper (II) nitrate
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Covalent or Ionic?
14b) tetraphosphorus hexoxide - P4O6
c) aluminum sulfate - Al2(SO4)3
d) Lead (IV) sulfite - Pb(SO4)2 (reduced)