Unit test #1

Question 1

Binary compounds

Answer 1

Metals that only have 1 charge
-metal-non,criss cross simplify Ex: Berylium oxide BeO

Question 2

Multivalent

Answer 2

-Metal has more ten 1 charge
-Roman numeral added
Ex: SnO2 Tin(IV) oxide

Question 3

Polyatomic

Answer 3

-ending=ate or ite
- use brackets around poly atom
- Cu(SO3) 2 Copper(II) sulfite

Question 4

Hydrate

Answer 4

-Water attacked to a crystal
-uses prefix to show the # of water molecules
-hydrate at the end of the name
Ex: CuSO4 . 5H2O
Copper(2) sulfate pentahydrate

Question 5

Ionic compounds (nomenclature) rules

Answer 5

• if metal is multivalent find charge mathematically
  1. eqaution= # of atoms of element x ion charge = total ion charge for anion
  Cu l O 1 x -2=-2 switch sides
  2/1= 2 Copper (II) oxide

Question 6

Anhydrous

Answer 6

is compound formed from the hydrates remains in water is removed Ex: CaCl2
CoCl2 . 6H20
- Write a dot in between compound to show association

Question 7

Acids

Answer 7

Binary: H + nonmetal or polyatomic ion that doesnt have O
1. H first then non metal
2. criss cross
3. Write (aq)
Ex: Hydrobromic acid
HBr(aq)
Oxyacid: H+ polyatomic ion with oxygen
1. H then polyatomic symbols
Note: -IC ending from ATE and OUS from ITE
2. criss cross cant be simplified
3.write aq
Ex; Chloric (ate) acid
HClO3 aq

Question 8

what are Molecular compounds

Answer 8

Made up of 2 or more non metals sharing electrons in covalent bonds to make full octets
-can be solid,liquid or gas , low melting point and boiling,not easily dissolved in water
-uses prefixes to name change nonmetal ending to IDE

Question 9

Electronegativity

Answer 9

The ability of an individual atom when bonded to attract bonding electrons to itself
- Higher the EN # the greated pull on shared electrons
- EN numbers can determine the type of bond (polar)

Question 10

EN

Answer 10

-must calculate if ionic or molecular
- Greater EN more likely a bond us to be ionic and an electron transfer
Ionic bond: metal + nonmetal electron transferred

Question 11

Polar covalent bond

Answer 11

• electrons spend more time with element with higher EN
• e- unequally shared
• • and - poles in a molecule
    + pole represented by Delta +
• pole represented by Delta -
  Highest EN - lowest EN to find polarity
  Ex:F-H
  4.0-2.1=1.9

Question 12

Non polar covalent bonds

Answer 12

• electrons are equally shared no poles
• EN must be less then 0.4 no deltas

Question 13

Lewis structures steps

Answer 13

1. Find a C.A (element with highest bonding capacity or lowest EN)
2. Tve- : Add all valence electrons
   if you have a polyatomic ion with a - charge u add 1 electron to your calculation if it has a + charge you take away an electron from calculation
3. Determine bond type by subtracting En for a polar or non polar bond
   (ionic bond electrons transfer non metal +metal)
   4.Draw the structure the bond represent 2 electrons if there is lone pairs on the C.A the structure bends.

Question 14

Molecular polarity

Answer 14

• If asymmetrical= polar molecule
• if symmetrical = non polar molecule
• even if symmetrical but not a polar bond(no deltas) still a non polar molecule

Question 15

Intermolecular forces

Answer 15

Forces of attraction b/w molecules

Question 16

Ionic compounds (intermolecular forces)

Answer 16

• not made up of molecules
• hold formula units of crystal (electrostatic attraction)
• Solids always at room temperature
• strong so have high MP/BP

Question 17

Molecular compounds

Answer 17

• strength of intermolecular forces determines physical properties (state of matter,MP/BP,surface tension)
• Room temp: mostly gases,few liquids(low BP) , solids melt easy means intermolecular forces are weak
• AS intermolecular forces increase in strength = MP/BP, surface tension increase

Question 18

LDF

Answer 18

• very weak attraction
• easily broken and made up again
• Exists in all molecules
• Cause: shift in electron cloud for fractions of a second in a molecule and creates a temporary dipole
• Temporary dipole also forms in neighboring molecule and they now attract to each other
• larger the molecule =more e- & p
• Stronger the force = high melting point

Question 19

Dipole Dipole

Answer 19

Force b/w oppositely charged ends of a polar molecule
Ex: H-Cl—–H-Cl (polar molecule)
- only seen in polar molecules
- Intermediate in strength
- the more polar the substance the stronger the dipole dipole force is
- these substances will have high BP/HP because of their intermediate strength

Question 20

Hydrogen bond

Answer 20

• Very strong force when H is bonded to only N,O,F
• large EN difference
• small size of H
  concentrates the positive pole which is able to easily
  attract a negative pole of another close molecule