Final Review 2013

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

Review

2a) Safety: -goggles -apron -closed toe shoes -hair tied back

Review

b) -follow directions -report accidents to teacher -place waste in designated containers -know the location of safety equipment -no horseplay

Review

c) Flush with water for 5 minutes

d) Rinse in safety shower (fully clothed)

Review

3. mass- electronic balance volume- graduated cylinder length – metric ruler time- stop watch temperature – thermometer

All measurements should have a NUMBER and UNIT!

SI Units for Measurements

a) Mass – gramsb) Volume – litersc) Length – meterd) Time – secondse) Temperature - ˚C

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

Reviewc) Percent error:

d) density:

e) quantitative data: numerical data (numbers)f) qualitative data: information describing color, odor, shape etc

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

% 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)

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

Density

8)

9)

70mL

2100gDensity = 30g/mL

20mL

75g

Density = 3.75g/mL

Density

10) 20/5 = 4g/mL B is the same

11) Read the BOTTOM of the meniscus

Volume is 43.0mL

Graphs13a) Pie graph- percentages b) Bar graph- comparisons

c) line graph- shows how the dependent variable changes with a change in the independent variable

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

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

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

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

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

Types of MixturesParticlessize

Tyndalleffect

Settling?

Solution tiny none noColloid small yes noSuspension large n/a yes

Tyndall effect b is a suspension

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

Types of Radiation

27a) Alpha beta gamma b)

c)

4 He2

0 β-1

0 ϒ0

Nuclear Equations

d) 226 222 Ra Rn + 88 86

ii) 14 14 C N + 6 7

4 He2

0 β-1

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

Half- Life

29) Time

(minutes)Amount (g)

0 16518 82.536 41.2554 20.6272 10.3190 5.16

Half- Life

29b)Time

(minutes)Amount (g)

0 10.01 5.02 2.50

Half-Life application30) Using C-14 to determine the age of a fossil

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.

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

Chapter 533) Get definitions from the textbook34) s, p, d, f

b)

Various shapes- spherical, dumbbell etc

Sublevels

c) Sub-Level

# electrons

s 2p 6d 10f 14

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

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-

Flame Tests

38) Elements give of distinct colors when heated in a flame. The color of the flame is matched to the known element.

Electron Configuration

39a) 4p1 – Gallium b) 5s2 – Strontium c) 6p6 – Radon d) 7s1 – Francium

40) Same column- similar ending config

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

Periodic Trends

c) Ionization Energy decreases down the group increases across

Lowest IE – Francium Highest IE - Helium

Periodic Trendsd) Electronegativity decreases down the group increases across

Lowest E – Francium Highest E - Fluorine

Periodic Trendse) Metals become SMALLER when they turn into ions

Non-metals become LARGER

Periodic Trends

f) Francium is most active metal. Fluorine most active non-metal.

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

AKS11b Metal/Nonmetal/Metalloida) Metals left, nonmetals right , metalloids

border the stairstep line. Stairstep line separates metals and nonmetals

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

Chapter 8 - Ionic Bonding

1. a)

b)

CaCl2

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

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

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

Chapt 9 - Covalent Bonding

6)

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

Lewis Structures

10a) b)

c) d)

e)

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

Covalent or Ionic?

14b) tetraphosphorus hexoxide - P4O6

c) aluminum sulfate - Al2(SO4)3

d) Lead (IV) sulfite - Pb(SO4)2 (reduced)