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
Rb
Ti
Kr
S
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
John Newlands (1863)
Law of octaves – properties repeat every 7
elements
Periodic Table
John Newlands (1863)
Periodic Table
John Newlands (1863)
Periodic Table
Mendeleev (1869)
• Dmitri Mendeleev – 1869
• Father of the Periodic Table
Periodic Table
Mendeleev (1869)
Periodic Table
Mendeleev (1869)
• Major Success - Left spaces where there
should be an element
Al
Si
Ga
In
P
As
Sn
Sb
Periodic Table
Mendeleev (1869)
Eka-Silicon - “below silicon”
Eka-Silicon(1871)
~72 g/mol
Density ~5.5 g/mL
Dark Gray Metal
EsO2 (4.7 g/mL)
Periodic Table
Mendeleev (1869)
Eka-Silicon(1871) Germanium(1886)
~72 g/mol
72.6 g/mol
Density ~5.5 g/mL 5.36 g/mL
Dark Gray Metal
Dark Gray Metal
EsO2 (4.7 g/mL)
GeO2 (4.7 g/mL)
(Scandium and Gallium predicted also)
Periodic Table
Periodic Table
Mendeleev (1869)
Modern Table -Different than Mendeleev’s
– Problem with Mendeleev’s table Arranged his table by atomic mass
– Modern table arranged by atomic number
(Moseley)
Periodic Table
Periodic Table
Metals
Properties
a. Solids
b. Ductile
c. Malleable
d. Conduct Electricity and heat
e. Large - Tend to lose electrons
Periodic Table
Periodic Table
Periodic Table
Periodic Table
Non-Metals
Properties
a.
b.
c.
d.
Gases or solids
Brittle
Don’t conduct Electricity & heat well
Essential for Life
CHONSP
e. Small - Tend to gain electrons
Periodic Table
Periodic Table
Periodic Table
Metalloids
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
Periodic Table
Periodic Table
Group Names
Period – Across
Group – Down
Periodic Table
Group Names
Periodic Table
States
• Standard Temperature = 25oC
• Solids – Most Elements
Liquids – Hg and Br2
Gases – H2, N2, O2, F2, Cl2
& Noble Gases
IA
IIA
IIIA
IVA
VA
VIA
VIIA
Carbide
C4-
Nitride
N3-
Oxide
O2-
Fluoride
F-
Phosphide
P3-
Sulfide
S2-
Chloride
Cl-
Hydride
HLithium
Li+
Beryllium
Be2+
Sodium
Na+
Magnesium
Mg2+
Potassium
K+
Calcium
Ca2+
Selenide
Se2-
Bromide
Br-
Rubidium
Rb+
Strontium
Sr2+
Telluride
Te2-
Iodide
I-
Cesium
Cs+
Barium
Ba2+
Aluminum
Al3+
Periodic Table
Cl
Cu2+
Na
Fe3+
Ba
SO42-
OH-
PO43-
Periodic Table
H He
Al
Periodic Table
No Roman # Ionics
I. Binary Compounds
A. Used for Gr 1 and Gr 2 metals (and
Aluminum)
B. Metal has only one standard charge
C. Rules
•
•
Write Metal First
Non-metal becomes “ide”
Periodic Table
No Roman # Ionics
D. Examples
NaCl
BaO
Al2O3
magnesium bromide
aluminum sulfide
potassium oxide
Periodic Table
No Roman # Ionics
II. Compounds with Polyatomics
A. Polyatomic Ion - An Ion with more than
one atom (Consider the overall charge)
B. Examples
Hydroxide
Nitrate
Sulfate
Acetate
Periodic Table
No Roman # Ionics
C. Examples
sodium hydroxide
sodium carbonate
aluminum sulfate
NaNO3
Ca(OH)2
(NH4)3PO4
D. Mixed Examples
magnesium sulfide
magnesium sulfite
magnesium sulfate
lithium phosphide
lithium phosphate
Ba(ClO3)2
BaCl2
Periodic Table
Roman # Ionics
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
Periodic Table
Roman # Ionics
3. The Roman Numeral tells you the charge, NOT
how many atoms you have.
copper(II)nitride
copper(III)nitride
Periodic Table
Roman # Ionics
4. Examples
iron (III)bromide
tin(II) nitrate
cobalt(III)oxide
CoCl2
MnO2
Ru2(SO4)3
VO3
Periodic Table
Roman # Ionics
5. Mixed Examples
calcium bromide
chromium (III)nitrate
aluminum sulfate
iron(III)carbonate
Li2S
CoCl2
Ti3N2
Mg(NO2)2
Periodic Table
Molecular Naming
1. Prefixes
Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
May skip “mono” for first element
Periodic Table
Molecular Naming
2. Examples
P4O10
SiO2
CO
diphosphorus tetroxide
carbon tetrachloride
dinitrogen tetroxide
dichlorine decoxide
carbon disulfide
sulfur hexafluoride
SeF4
Cl2O7
KrF4
CH4
Periodic Table
Rev. of All Naming
calcium chloride
silicon dioxide
copper(II)carbonate
magnesium phosphate
dicarbon octahydride
chromium(III)oxide
dihydrogen monsulfide
Periodic Table
Oxidation 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
Table
Elements = 0
Fe
H2 P4
Cl2
Monoatomic Ions
= Charge
Na+ O2- Al3+
Use “bankables” to
calculate the rest
H2S Cl2O
PO43-
Na2SO4
NO3-
CaCr2O7 SnBr4
Gr I
Gr II
O-2
H+
F-
“the higher the oxidation #, the more oxidized the element”
Calculate the oxidation numbers for:
HClO
S8
Mn2O3
KMnO4
Cr3+
SO32HSO4NO2SO42Fe2(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.
2.
3.
4.
5.
V2O5
XeCl4
Ca(NO3)2
Barium nitride
Iron(III)carbonate
10. Ne, Cl2, N2
11.a) N2
d) F2
e) H2
12. Ru, Sn, Hf, W
13.Te and B
14.A) Ar b) Hg c) N2 d) Be
15.a) Br2
b) Ar
c) I2
h)Hg2
e) Bi
d)H2 or C
18.Lithium fluoride
strontium nitride
aluminum chloride
19. calcium iodide
francium fluoride
beryllium selenide
20. Rb2Se SrH2 RaO
21.KH
Cs2S
23. chromium (III) iodide
iridium(VIII) oxide
nickel(II) chloride
barium telluride
barium hydride
magnesium phosphide
radium sulfide
Al3C4 BeF2
K 3P
BaTe
titanium(IV) chloride
manganese(II) hydride
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
SiO2
NaNO3
Na3N
Al2(SO4)3
Al2S3
Fe2(SO4)3
Li3PO4
Cu(C2H3O2)2
Cu2O
chromium(III)carbonate
copper(II)nitrate
copper(II)nitrite
dinitrogen pentoxide
nickel(II) bicarbonate
tin(II) bromide
aluminum fluoride
potassium permanganate
chlorine dioxide
potassium chromate
ammonium carbonate
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