Periodic Table/trends

Question 0

Henry Moseley

Answer 0

Was 1st to arrange elements in a table format by atomic NUMBER

Question 1

Dimitri Mendeleev

Answer 1

Produced 1st periodic table

• arranged elements according to atomic MASSES
• his table had empty spaces for elements yet to be discovered

Question 2

Periodic law

Answer 2

When elements are arranged by atomic number, similar properties will exist in every 8 or so elements

Question 3

Rows are called

Answer 3

Periods

Question 4

Columns are called

Answer 4

Families or groups

Question 5

Alkali metals

Answer 5

• 1st column/group
• reactive with water and air
• generally a 1+ charge
• soft metals (can cut with a butter knife)
• forms basic solutions

Question 6

Alkaline earth metals

Answer 6

• 2nd column/group
• not as reactive as Alkali metals
• generally 2+ charge
• also somewhat soft metals
• forms basic solutions

Question 7

Halogens

Answer 7

• 2nd last column/group
• very reactive non-metals
• generally a -1 charge
• F (g) Cl (g) Br (l) I (s) At (s) diff. phases
• forms acidic solution

Question 8

Noble gases

Answer 8

• generally non-reactive (inert) gases
  (some exceptions)
• full outer shell

Question 9

Transition metals

Answer 9

• d block
• metals in this group have MANY different charges
• results in colored solution
• tend to form metal complexes w/ certain ligands (attachments)

Question 10

Metallic properties

Answer 10

Shiny, luste, malleable, ductile, conductive ect.

|———–non-metal
| I
|. I
Metal——————

Question 11

Atomic size (radii)

Answer 11

• going down a column INCREASES atomic size. (orbitals get larger)
• going across from Left to Right, atomic size DECREASES
  - if # protons increases it leads to a greater nuclear charge; can attract electrons closer in

Question 12

Ion size (compared to neutral atoms)

Answer 12

• anions (-) will be LARGER than their neutral atom
  - more e. w/ same # protons; smaller pull per e.
• cations (+) will be SMALLER than their neutral atom
  - fewer e. w/ same # protons; greater pull per e.

Question 13

Ionization energy (IE)

Answer 13

• energy required to remove an outermost e. from a atom
  - 1st IE -> energy required to remove first outermost e.
  
  • 2nd IE -> energy required to remove second outermost e.

DECREASES going down
- because e. are farther away from nucleus
INCREASES left to right
- because of greater nuclear charge (larger pull)

Question 14

Electronegativity

Answer 14

• the ability of a nucleus to attract electrons towards its self WITHIN A BOND

DECREASES going down

   - outermost e. is further away
         - > Shielding effect 

INCREASES going left to right
- more protons; greater nuclear pull

Question 15

Shielding effect

Answer 15

Inner e. will “shield” away some of the nuclear pull towards outer e.

Question 16

Remember:

Answer 16

SIZE OVERPOWERS, # protons in the nucleus
- look at size first

Look up/down before left/right

These are trends - many exceptions exist

Question 17

Lanthanides/Actinides

Answer 17

Radioactive

Question 18

Radioactive elements

Answer 18

Lanthanides

Actinides

Question 19

Types of chemical bonding

Answer 19

Ionic, covalent, polar covalent

Question 20

Ionic bonds

Answer 20

Results from the electrostatic attraction between cations and anions

Question 21

Mechanism of ionic bonds

Answer 21

1) an atom (usually a metal) transfers electron(s) to another atom (usually a non metal)
2) the atom that lost e. becomes + charged (cation) while the atom that gained e. becomes - charged (anion)
3) the cation will be attracted to the anion through electrostatic attraction (opposite charges attract)

Question 22

Covalent and polar covalent similarities

Answer 22

Arise from a sharing of e.

Question 23

Covalent and polar covalent defferences

Answer 23

Pure covalent

• equal sharing of the bonding pair of e.
• similar Electronegativity values

Polar covalent

• unequal sharing of the bonding pair e.
• sig. Different Electronegativity values between atoms

Question 24

Polar covalent

Answer 24

- unequal sharing of the bonding pair e. | - sig. Different Electronegativity values between atoms

Question 25

Pure covalent

Answer 25

Pure covalent - equal sharing of the bonding pair of e. - similar Electronegativity values

Question 26

Its ionic if the Electronegativity value is

Answer 26

Greater than 1.7

Question 27

It's polar covalent if the Electronegativity value is

Answer 27

Between 0.5 and 1.7

Question 28

It's pure covalent if the Electronegativity value is

Answer 28

Less than 0.5

Question 29

In a covalent compound which atoms MUST Have 8 e around them

Answer 29

C, N, O, F

Question 30

Which atom only needs 6 e.

Answer 30

B

Question 31

VSEPR stands for

Answer 31

Valence Shell Electron Pair Repulsion

Question 32

Polarity of molecules

Answer 32

If these polar bonds in a molecule do NOT cancel each; then the molecule is considered polar (net dipole)

Question 33

Noun of polar

Answer 33

Net dipole

Question 34

Solubility - like dissolves like

Answer 34

Non-polar solutes dissolve in non polar solvents polar solutes dissolve in polar solvents

Question 35

What VSEPR shapes are always polar (due to the location of the lone pairs)

Answer 35

``` Bent/angular Trigonal pyramid Seesaw T shape Square pyramid ```

Question 36

Intermolecular forces (IHF)'s

Answer 36

Attractions BETWEEN molecules

Question 37

Intramolecular forces

Answer 37

Ionic, covalent and polar covalent | within

Question 38

6 types of Intermolecular forces (IHF's) Weakest to strongest

Answer 38

1. London Dispersion forces/Van der Waals forces 2. Dipole - Dipole attractions 3. Hydrogen Bonding 4. Metallic bonding 5. Ionic Lattice structures 6. Covalent network solids

Question 39

London dispersion forces/ Van der Waals Forces

Answer 39

Weakest - attractions that arise form TEMPORARY dipoles in molecules - exist for all chemical species

Question 40

Dipole - Dipole attractions

Answer 40

2nd weakest - exist between POLAR MOLECULES (ie. have PERMANENT dipole) - therefor it's a bit stronger than LD forces

Question 41

Hydrogen bonding

Answer 41

3rd weakest - attraction between H of one molecule and a lone pair of a N, O, F Atom of a second molecule

Question 42

Metallic Bonding

Answer 42

4th weakest Metal atoms are attracted to each other and can pass e. around (explains why metals are good conductors)

Question 43

Ionic lattice structure

Answer 43

- recall: ionic compounds exist as crystal lattices | - atoms in this structure are STRONGLY attracted to each other

Question 44

Covalent network solids

Answer 44

- like ionic lattices but w/ covalent bonds Ex. Carbon (graphite), Carbon (diamond), SiO2 (quartz) Sometimes: metal carbides and silicides

Question 45

Connection to KMT/ boiling melting point

Answer 45

- energy required to melt/boil a substance is used to counteract the IMF's present - substances with STRONG IMF will have HIGH melting/boiling point