1.A cylinder of copper (8.92 g/cm 3 ) is found to have a mass of 1681 grams. a.The cylinder is 15.0...
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Transcript of 1.A cylinder of copper (8.92 g/cm 3 ) is found to have a mass of 1681 grams. a.The cylinder is 15.0...
1. A cylinder of copper (8.92 g/cm3) is found to have a mass of 1681 grams.a. The cylinder is 15.0 cm tall. Calculate the radius. (2.0cm)b. A rectangular piece of copper has a mass of 0.330 kg. The
dimensions are 1.00 cm and a width of 4.000 cm by 9.000 cm. Calculate the experimental density.(9.17g/cm3)
c. Calculate the percent error. (2.8%)
2. 1220 J of heat is added to 50.0 grams of water at 25.0oC. a. Calculate the change in temperature of the water. (5.8oC)b. Calculate the final temperature of the water. (30.8oC)c. Convert the heat to kilojoules. (1.22 kJ)d. Convert the heat to calories. (292 cal)
1. What type of element is:
Ba Br Th S
Rb Ti Kr Ce
2. What year did Mendeleev publish his periodic table?
3. How is the modern table different than Mendeleev’s?
4. Why do metals conduct and non-metals do not?
Periodic Table
Law of octaves – properties repeat every 7 elements
John Newlands (1863)
Periodic TableJohn Newlands (1863)
Periodic TableJohn Newlands (1863)
Periodic Table
• Dmitri Mendeleev – 1869
• Father of the Periodic Table
Mendeleev (1869)
Periodic TableMendeleev (1869)
Periodic Table
• Major Success - Left spaces where there should be an element
Mendeleev (1869)
Al Si P
Ga As
In Sn Sb
Periodic Table
Eka-Silicon - “below silicon”
Eka-Silicon(1871)
~72 g/mol
Density ~5.5 g/mL
Dark Gray Metal
EsO2 (4.7 g/mL)
Mendeleev (1869)
Periodic Table
Eka-Silicon(1871) Germanium(1886)
~72 g/mol 72.6 g/mol
Density ~5.5 g/mL5.36 g/mL
Dark Gray Metal Dark Gray Metal
EsO2 (4.7 g/mL) GeO2 (4.7 g/mL)
(Scandium and Gallium predicted also)
Mendeleev (1869)
Periodic Table
Periodic Table
Modern Table -Different than Mendeleev’s
– Problem with Mendeleev’s table - Arranged his table by atomic mass
– Modern table arranged by atomic number (Moseley)
Mendeleev (1869)
Periodic Table
Periodic Table
Propertiesa. Solids b. Ductilec. Malleabled. Conduct Electricity and heate. Large - Tend to lose electrons
Metals
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Propertiesa. Gases or solids
b. Brittle
c. Don’t conduct Electricity & heat well
d. Essential for Life
CHONSP
e. Small - Tend to gain electrons
Non-Metals
Periodic Table
Periodic Table
Periodic Table
Properties
a. Have properties of both metals and non-metals
b. Semi-Conductors - Conduct electricity only if a larger current is applied
c. Used in computer chips, cell phones, etc…
d. B, Si, Ge, As, Sb, Te
Metalloids
Periodic Table
Periodic Table
Period – AcrossGroup – Down
Group Names
Periodic TableGroup Names
Periodic Table
• Standard Temperature = 25oC
• Solids – Most Elements
Liquids – Hg and Br2
Gases – H2, N2, O2, F2, Cl2
& Noble Gases
States
IA IIA IIIA IVA VA VIA VIIA
HydrideH-
LithiumLi+
BerylliumBe2+
CarbideC4-
NitrideN3-
OxideO2-
FluorideF-
SodiumNa+
MagnesiumMg2+
AluminumAl3+
PhosphideP3-
SulfideS2-
ChlorideCl-
PotassiumK+
CalciumCa2+
SelenideSe2-
BromideBr-
RubidiumRb+
StrontiumSr2+
TellurideTe2-
IodideI-
CesiumCs+
BariumBa2+
Periodic Table
Cl SO42- OH- PO4
3-
Cu2+
Na
Fe3+
Ba
Periodic Table
H He
Al
Periodic Table
I. Binary CompoundsA. Used for Gr 1 and Gr 2 metals (and
Aluminum)B. Metal has only one standard chargeC. Rules
• Write Metal First• Non-metal becomes “ide”
No Roman # Ionics
Periodic Table
D. Examples
NaCl
BaO
Al2O3
magnesium bromide
aluminum sulfide
potassium oxide
No Roman # Ionics
Periodic Table
II. Compounds with Polyatomics
A. Polyatomic Ion - An Ion with more than one atom (Consider the overall charge)
B. ExamplesHydroxide Sulfate
Nitrate Acetate
No Roman # Ionics
Periodic Table
C. Examplessodium hydroxide
sodium carbonate
aluminum sulfate
NaNO3
Ca(OH)2
(NH4)3PO4
No Roman # Ionics
D. Mixed Examples
magnesium sulfide
magnesium sulfite
magnesium sulfate
lithium phosphide
lithium phosphate
Ba(ClO3)2
BaCl2
Periodic Table
1. An example
Fe(II)and oxygen
Fe(III) and oxygen
How do we distinguish?
2. Metals which have multiple oxidation states
Transition and post-transition metals
Roman # Ionics
Periodic Table
3. The Roman Numeral tells you the charge, NOT how many atoms you have.
copper(II)nitride
copper(III)nitride
Roman # Ionics
Periodic Table
4. Examplesiron (III)bromide
tin(II) nitrate
cobalt(III)oxide
CoCl2
MnO2
Ru2(SO4)3
VO3
Roman # Ionics
Periodic Table
5. Mixed Examplescalcium bromidechromium (III)nitratealuminum sulfateiron(III)carbonate
Li2S
CoCl2
Ti3N2
Mg(NO2)2
Roman # Ionics
Periodic Table
1. PrefixesMono HexaDi HeptaTri OctaTetra NonaPenta Deca
May skip “mono” for first element
Molecular Naming
Periodic Table
2. Examples
P4O10
SiO2
CO
diphosphorus tetroxide
carbon tetrachloride
Molecular Naming
dinitrogen tetroxide
dichlorine decoxide
carbon disulfide
sulfur hexafluoride
SeF4
Cl2O7
KrF4
CH4
Periodic Table
calcium chloride
silicon dioxide
copper(II)carbonate
magnesium phosphate
dicarbon octahydride
chromium(III)oxide
dihydrogen monsulfide
Rev. of All Naming
Periodic TableOxidation Numbers
1. Involves taking compounds apart
2. Oxidation numbers – Pretend charges for all compounds (as if they exist as a monoatomic ion)
3. Rules
Periodic TableElements = 0
Monoatomic Ions = Charge
Use “bankables” to calculate the rest
Gr I Gr II
O-2 H+ F-
Fe H2 P4 Cl2
Na+ O2- Al3+
H2S Cl2O Na2SO4
PO43- NO3
-
CaCr2O7 SnBr4
“the higher the oxidation #, the more oxidized the element”
Calculate the oxidation numbers for:
HClO SO32-
S8 HSO4-
Mn2O3 NO2-
KMnO4 SO42-
Cr3+ Fe2(SO4)3
More Oxidation Number Examples:
NaClO
Fe2S3
KIO4
H2PO4-
C2H3O2-
CS2
N2O
NaI
K2CO3
HgI2
FeF2
PCl5
NO3
Ba(OH)2
Periodic Table
1. V2O5
2. XeCl4
3. Ca(NO3)2
4. Barium nitride
5. Iron(III)carbonate
10. Ne, Cl2, N2
11.a) N2 d) F2 e) H2 h)Hg2
12. Ru, Sn, Hf, W
13.Te and B
14.A) Ar b) Hg c) N2 d) Be e) Bi
15.a) Br2 b) Ar c) I2 d)H2 or C
18.Lithium fluoride barium telluride
strontium nitride barium hydride
aluminum chloride
19. calcium iodide magnesium phosphide
francium fluoride radium sulfide
beryllium selenide
20. Rb2Se SrH2 RaO Al3C4 BeF2
21.KH Cs2S K3P BaTe
23. chromium (III) iodide titanium(IV) chloride
iridium(VIII) oxide manganese(II) hydride
nickel(II) chloride
23. chromium (III) iodide titanium(IV) chloride
iridium(VIII) oxide manganese(II) hydride
nickel(II) chloride
25. YH3 BiF5
PbCl4 PdSe
25. YH3 BiF5
PbCl4 PdSe
33.sodium oxalate calcium chromate
iron(III) carbonate copper(II) hydroxide
34. Mg(MnO4)2 Co(CN)2 Sr(OH)2
Th2SO3 Fe2(C2O4)3 (NH4)2Cr2O7
Hg2(C2H3O2)2
35.Zr3(PO4)4 NaCN TlNO2
Ni(OH)2 Ra(HSO4)2 Be3(PO4)2
Cr(ClO)3
MgO Al2S3
SiO2 Fe2(SO4)3
NaNO3 Li3PO4
Na3N Cu(C2H3O2)2
Al2(SO4)3 Cu2O
chromium(III)carbonate aluminum fluoride
copper(II)nitrate potassium permanganate
copper(II)nitrite chlorine dioxide
dinitrogen pentoxide potassium chromate
nickel(II) bicarbonate ammonium carbonate
tin(II) bromide carbon tetrafluoride
Ionic (No Roman #)
Sodium fluoride (NaF)
Lithium phosphate (Li3PO4)
Sodium carbonate (Na2CO3)
Aluminum sulfide (Al2S3)
Barium nitrate (Ba(NO3)2)
Sodium bicarbonate (NaHCO3)
Barium nitride (Ba3N2)
Potassium hydrogen sulfate (KHSO4)
Potassium permangante (KMnO4)
Sodium hydroxide (NaOH)
Ionic (Roman # needed)
Iron(III) oxide (Fe2O3)
Chromium(III) hydroxide (Cr(OH)3)
Titanium(IV) oxide (TiO2)
Manganese(IV) oxide (MnO2)
Zinc(II) chloride (ZnCl2)
Iron(II) oxide (FeO)
Lead(II) chloride (PbCl2)
Cobalt(II) chloride (CoCl2)
Copper(II) fluoride (CuF2)
Molecular (Prefixes)
Nitrogen trihydride (NH3)
Carbon monoxide (CO)
Diphosphorus pentoxide (P2O5)
Dioxygen difluoride (O2F2)
Nitrogen monoxide (NO)
Dicarbon tetrahydride (C2H4)
Dinitrogen tetroxide (N2O4)
1) a) Pb(+2) b) P(+5) c) C(-1) d) N(+2)
e) H(-1) f) B(+3) g) Se(-2) h) Bi(+3)
2) a) Cl(+4) b) Xe(+2) c) C(+2) d) O(+1)
e) Mn(+3) f) Bi(+5)
6) a) +5 b) +3 c) +7 d) +6 e) +6
f) +5 g) +7
7) a) +6 b) +3 c) +6 d) +5 e &f) +6
8.a) +4 b) +7 c) +4 d) +3 e) -3
• Non-metals can be + or –
• Metals can only be +
• Transition metals often are +2, +3
• Increase by one as you go across horizontal
• +7 usually the highest
• Often decrease by 2 for an element