Niche things to remember

Hydrochloric acid

HCl

Hydrobromic acid

HBr

Hydroiodic acid

HI

Nitric acid

HNO3

Sulfuric acid

H2SO4

Chloric acid

HClO3

Perchloric acid

HClO4

Roman numerals

1. Mono = 1

2. Di = 2

3. Tri = 3

4. Tetra = 4

5. Penta = 5

6. Hexa. = 6

7. Hepta. = 7

8. Octa. = 8

9. Nona. = 9

10. Deca. = 10

The chargers to always remember

1. Remember Ag (transition metal) is always +1

2. Remember Cd (transition metals) is always +2

3. Remember Zn (transition metals) is always +2 

4. Remember Al (transtion metal) is always +3

The roman numerals

1. I  = +1

2. II  = +2

3. III  = +3

4. IV = +4 

5. V = +5

6. VI = +6

7. VII = + 7

CCMAA rule for electron configuration

This is the rule for transition metals and it states that for the transition metals:

1. Cu

2. Cr

3. Mo

4. Au

5. Ag

the electrons in the last 3 orbitals will jump to the last d orbitals to allow it to be filed with 5 electrons or fully filled with 10 electrons (if it can’t achieve that it will not)

Valence electrons for the transition metals (3-12)

include the electrons in the outermost energy level and the closet d orbital

Exception to ionization energy

This is the amount of energy it takes for an electron to become an ion (so it is an endothermic process), and the more energy it takes the less than an electron wants to give up it’s electrons:

1. It increases from left to right across a period

2. it decreases down each period

The exceptions include

1. Beryllium and boron (as Beryllium has. higher ionization energy) (this is due to it’s filled 2s² orbitals adverse to borons unfilled 2p^1 orbitals, that has more energy because the p can’t penetrate as well)

2. Nitrogen and oxygen (nitrogen has. higher ionization energy because it configuration of 2p³ allows for less electron-electron repulsion adverse to oxygen 2p^4 allow for more electron electron repulsion)

This occurs for all the element in the 2a and 3a group

This occur for all the element in-group 5A and 6A

Valence bond theory

Remember for this theory when you are trying to figure our the hybridized for an atom, you would count both its lone pairs in the electron group, and when you are trying to find out the electron geometry (apart of the VSPER theory) you would include the loner Paris

Writing lewis structures

Remember that for writing theses Group 15, 16, 17, and 18 have the ability to have expanded octet (but only for nonmetals, and are at and below period 3)

1. Group 15: Can form 5 bonds (10 electrons)

2. Group 16: Can form 6 bond (12 electrons)

3. Group 17: Can form 6-7 bonds (12 - 14 electrons)

4. Group 18: Can form 6-7 bonds (12 - 14 electrons)

Linear (electron geometry and molecular geometry)

This would have:

1. 2 electron groups

2. 2 bonding groups

3. 0 lone Paris

Its approximate bond angles would be 180

Trigonal Planar

This would have:

1. 3 electron groups

2. 0 lone paris (120 degrees)

   1. Would still be trigonal planar

3. 1 lone pair

   1. Would be bent (<120 degrees)

Tetrahedral

This would have:

1. 4 electron groups

   1. 0 lone paris

   2. Tetrahedral (109.5 degrees)

2. 4 electron groups

   1. 1 lone paris

   2. trigonal pyramidal (< 109.5 degrees)

3. 4 electron groups

   1. 2 lone pairs

   2. bent ( < 109.5 degrees)

Trigonal bipyramidal

1. 5 electron groups

   1. 0 lone groups

   2. trigonal bipyramidal (120 degrees equatorial, 90 degree axial)

2. 5 electron groups

   1. 1 lone pair

   2. seesaw (< 120 degrees equatorial, <90 degrees axial)

3. 5 electron groups

   1. 2 lone pairs

   2. t-shaped (< 90 degrees)

4. 5 electron groups

   1. 3 lone pairs

   2. linear (180 degrees)

Octahedral

1. 6 electron groups

   1. 0 lone pairs

   2. octahedral (90 degrees)

2. 6 electron groups

   1. 1 lone pairs

   2. square pyramidal (less than 90 degrees)

3. 6 electron groups

   1. 2 lone pairs

   2. square planar (equal to 90 degrees)

Placing hydrogen in a covalent bond

1. Hydrogen goes first with group 16 and group 17 (except oxygen)

2. Hydrogen goes second with Carbon (CH) and nitrogen (NH)

3. hydrogen goes second with boron and silicon (BH) and (SiH)

4. It was always (CHO)

Bond polarity on the Pauling scale

1. (0 - 0.4 ) small electronegativity difference so it is still a covalent bond

2. (0.4 - 2.0 ) intermediate electronegativity difference, it is apolar covalent bond (with partial negative and partial positive charge)

3. (2.0 +) large ionic bond

Mass percent

(total mass of that compound in a given compound) / (the molar mass of the compound that we have) * 100

How to draw the structural formual

1. mirror lewis structures just without the lone Paris

2. don’t follow VESPR theory unless told to

Octet rule exceptions

1. helium and hydrogen form an octet

2. Lithium (2s^1 loses on electron to be stable) (mirror He Nobel gas)

3. Be (2s² loses two election to the stable) (minor the He Nobel gas)

   1. doesn’t form a covalent bond because it is a metal

4. Boron (2s² 2p^1 loses three electron to mirror He Nobel gas, when it form a covalent bond it is stable with 6 valence electrons

Writing out chemical formulas

1. Write the cation first and then the anion (so the metal first and then the nonmetal)

2. The sum of the chargers have to cancel out 

   1. Remember Ag (transition metal) is always +1

   2. Remember Cd (transition metals) is always +2

   3. Remember Zn (transition metals) is always +2 

   4. Remember Al (transition metal) is always +3

3. Formula has to contain the smallest whole number ratio of ions

Writing out names for ionic compounds

1. Name the cation first (metal or polyatomic cation)

2. State the metal’s oxidation state (so the amount of electrons it has lost) as a roman numeral in parenthesis

   1. Except Group I / II metals 

   2. Group 1 metals will always have a +1 charge (s^1)

   3. Group 2 metals will always have a +2 charge  (s^2)

Water of hydration

1. Water of hydration

   1. Tells you how many water molecules are incorporated in a formula unit for an ionic compound 

   2. Name the ionic compound that add prefixes to indicate how many and then hydrate

How to name molecular compoudns

1. Start with the most metallic character first 

   1. So left most on the same row 

   2. Or if they are in the same group the ones that have the higher row number (so more down)

   3. Then you would leave the first atom name unchanged

   4. The you would change the second atom name to end in -ide

   5. You would add prefixed to indicate the amount 

      1. DTT PHH NOD

         1. Di

         2. Tri

         3. Tetra 

         4. Penta 

         5. Hexa 

         6. Hepta 

         7. Nona

         8. Octa

         9. Deca

   6. You would omit Mono if included

How to write molecular chemical formula (the molecular formula)

1. How to write molecular chemical formula (the molecular formula)

   1. Understand the prefixed

   2. Understand how the metallic atom has to go first