Module 6
What is the electron configuration of P?
1s2 2s2 2p6 3s2 3p3
What is an anion? Charge?
What is a cation? Charge?
Anion = element that takes e's.... - charge
Cation = element that gives up e's..... + charge
What type of bond is formed by 1 metal and 1 nonmetal?
IONIC
What is an empirical formula?
It is the simplest ratio/form that a compound can have
What is Ms. Chase's favorite color?
Blue!!
What is the abbreviated electron configuration of P?
[Ne] 3s2 3p3
Cl with 7 valence e around it
What type of bond is formed by 2 nonmetals?
Covalent
CH7 = empirical or molecular?
C7H14 = empirical or molecular?
Empirical
Molecular
Write an example of a molecular formula.
Answers vary.
How many valencene e's are in the following:
1. C
2. Xe
3. Cl
4. N
1. 4
2. 8
3. 7
4. 5
SHOW WORK
Convert 45g of Carbon to moles.
mass of C = 12.01 g
Convert 4 moles of C to g
45g C x (1 mole/12.01g) = 3.75 mol C
4 mol C x (12.01gC / 1 mol) = 48.04 mol C
2 metals
You have the compound C2H3 with a molecular mass of 81g/mol. What is the molecular formula?
Mass of C2H3 = 27g/mol
81/27 = 3
C2H3 x 3 = C6H9
What elements have the highest electronegativity?
Elements in the top right. Electronegativity increases as you move right and up across the periodic table.
Using the 4d10:
Which part of the symbol represents...
orbital?
energy level?
# of electrons in orbital?
orbital = d
energy level = 4
# of e in orbital = 10
Draw the electron dot structure of water.
H = 2 valence e max
O = 8 valence e
Draw answer on whiteboard
Write the name of the following:
N2O
N2O5
Write the symbols for the following:
carbon tetrachloride
triphosphorous hexafluoride
- dinitrogen monoxide
- dinitrogen pentoxide
CCl4
P3F6
How can you tell if something is empirical or molecular?
If it is empirical, then the ratios cannot be reduced any more.
If it molecular, you can reduce the numbers into a simpler form.
What type of bond is formed by 2 metals?
NON POLAR covalent
How many electrons can the following orbitals hold?s
s
p
d
f
s = 2
p = 6
d = 10
f = 14
Avogadro's # = 6.02x 10^23
56g C x (1mol/12.01g) = 4.66 mol C
4.66 mol x (6.02 x 10^23 / 1 mol) =
2.8 x 10^24 molecules of C
Write the formula for the following:
USE CHART IN CANVAS
1. CuSO3
2. Ba3 (AsO4)2
1. Copper (II) Sulfite
2. Barium arsenate
You have 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen. What is the empirical formula?
40g C x (1 mol C / 12.01g) = 3.33mol C
6.7g H x (1mol H / 1.001g) = 6.7 mol H
53.3 g O x (1mol O / 16.0g) = 3.33 mol O
6.7 / 3.33 = 2.... 2 H for 1 C and O
formula = CH2O
Tell me 3 trends that you can notice by looking at the periodic table.
electronegativity
metals vs. nonmetal
cations vs. anions