Chemistry Week 3

Periodic Table Group

• Vertical columns on the periodic table

• All elements have same number of valance electrons and core charge

• Elements inside a group have different properties but due to their identical number of valance electrons react similarly

Core charge

• Calculated by Z value - core electrons

Periodic Table Period

• Horizontal rows

• All elements have the same number of core electrons and shells

• If shell empty the shell disappears

Octet Rule

• Elements react in a way that gives them 8 valance electrons

• 8 valance electrons is identical to a noble gas

• This rule only applies to C, N, O, and F

• All the rest of the element try to match the valance electrons of the nearest noble gas

Ionic Compounds

• Type of bionic compound

• Always involves a Cation and Anion

• Always between a metal and non-metal

• Electrons are transferred from 1 element to the other

• Metals tend to loose their electrons

• Nonmetals tend to gain their electrons

Electrostatic Force

• Part of ionic bonding

• Attractive or repulsive force between two electrical charged objects

Lattice Energy

• Part of ionic bonding

• Energy contained in a crystal lattice

Coulomb’s Law

• Used to determine attraction between two ions

• If formula results in negative number the reaction will happen spontaneously

• r = size of the atom, found by looking at how many electron shells it has

• q1 = Charge of the first ion in the bond

• q2 = Charge of the second ion in the bond

Molecular Substance

Ex: Individual ice molecules being able to be identified in a lattice of ice

Covalent Bonding

• Type of binary compound

• Always between two non-metals and or metalloids

• A chemical bond involving sharing electrons between atoms

• However many electrons an atom wants to reach it’s nearest noble gas is how many bonds it will make with other atoms

- Ratios for pairing can not be scaled due to physical limitations with the molecular shape

Water

• Common chemical bond

• (H2O)

Ammonia

• Common chemical bond

• (NH3)

Calomel

• Common chemical bond

• (Hg2Cl2)

Binary Compounds

• Compound consisting of two elements

• Subdivided into Binary ionic compounds and Binary covalent compounds

Binary Ionic compounds

• Compounds consist of a metal and nonmetal

• Electron is donated

Binary covalent compounds

• Compounds consisting of nonmetals and or metalloids

• Shair electrons

mono-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 1

di-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 2

tri-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 3

• Word association: Tricycle

tetra-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 4

penta-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 5

• Word association: Pentagon

hexa-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 6

• Word association: Hexagon

hepta-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 7

octa-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 8

• Word association: Octagon

nona-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 9

deca-

• Greek prefix

• Used when naming binary covalent compounds to show how many atoms of each type there are

• Means 10

• Word association: Decade

Naming Ionic Compounds

• Name consists of two ion names, the metal one always lister first

• Metal ion: Based off of element name (doesn’t change from original element name)

• Nonmetal ion: Element name with the suffix of “-ide” added

• The metal has same ionic charge in all compounds: Name of the metal is just the original name of the metal

Ex: Lithium chloride (LiCl)

• The metal does not have the same ionic charge in all compounds (systematic names): Indicate the charge of the metal with a roman numeral in parentheses following the metal name

Ex: Iron(III) chloride (FeCl2)

• The metal does not have the same ionic charge in all compounds (older system names): When an Ion appears in two charges -ous is used to show the one of low charge and -ic is used to show the one of a higher charge

Ex: Ferrous chloride (FeCl2) or Ferric chloride (FeCl3)

Naming Covalent compounds

• Name consists of two ion names, the less electronegative element first

• The second ion takes on the suffix -ide

• A prefix is used to show the subscript of both elements

• If the first element’s prefix is “mono-” is is left off

Ex. Sulfur hexafluoride

Naming Polyatomic Compounds

• Same as ionic compounds

• The second name is just the name of the polyatomic ion

Ex: Sodium nitrite (NaNO2)

Naming Acids

• Follow two different naming rules

• Rule 1: When solid named same as binary or polyatomic ions compounds

• Rule 2: When dissolved in water follow below rules

• Substance does not contain oxygen: Add prefix “hydro-” and the suffix “-ic acid” to the name of the non-hydrogen part or polyatomic ion

Ex: HF Hydrofluoric acid

• Substance does contain oxygen (all that contain oxygen are polyatomic compounds) and the anion ends with the suffix “-ite”: Replace “-ite” with “-ous”

Ex: Sulfurous acid (H2SO3) “Sulfite” is being turned to “Sulfurous”

• Substance does contain oxygen (all that contain oxygen are polyatomic compounds) and the anion ends with the suffix “-ate”:

Ex: Sulfuric acid (H2SO4) “Sulfate” is being changed to “Sulfuric”

Acid

• Simplified def. for purpose of this class: An acid is any substance that dissolves in water to yield H+ ion.

(aq)

• Notation meaning that the result is aqueous

(S)

• Notation meaning that the result is a solid

(L)

• Notation meaning that the result is a liquid

(G)

• Notation meaning that the result is gas

Hydrogen

• Periodic Element

• Atomic Number: 1

• Symbol: H

Helium

• Periodic Element

• Atomic Number: 2

• Symbol: He

Lithium

• Periodic Element

• Atomic Number: 3

• Symbol: Li

Beryllium

• Periodic Element

• Atomic Number: 4

• Symbol: Be

Boron

• Periodic Element

• Atomic Number: 5

• Symbol: B

Carbon

• Periodic Element

• Atomic Number: 6

• Symbol: C

Nitrogen

• Periodic Element

• Atomic Number: 7

• Symbol: N

Oxygen

• Periodic Element

• Atomic Number: 8

• Symbol: O

Fluorine

• Periodic Element

• Atomic Number: 9

• Symbol: F

Neon

• Periodic Element

• Atomic Number: 10

• Symbol: Ne

Sodium

• Periodic Element

• Atomic Number: 11

• Symbol: Na

Magnesium

• Periodic Element

• Atomic Number: 12

• Symbol: Mg

Aluminum

• Periodic Element

• Atomic Number: 13

• Symbol: Al

Silicon

• Periodic Element

• Atomic Number: 14

• Symbol: Si

Phosphorus

• Periodic Element

• Atomic Number: 15

• Symbol: P

Sulfur

• Periodic Element

• Atomic Number: 16

• Symbol: S

Chlorine

• Periodic Element

• Atomic Number: 17

• Symbol: Cl

Argon

• Periodic Element

• Atomic Number: 18

• Symbol: Ar

Potassium

• Periodic Element

• Atomic Number: 19

• Symbol: K

Calcium

• Periodic Element

• Atomic Number: 20

• Symbol: Ca

Scandium

• Periodic Element

• Atomic Number: 21

• Symbol: Sc

Titanium

• Periodic Element

• Atomic Number: 22

• Symbol: Ti

Vanadium

• Periodic Element

• Atomic Number: 23

• Symbol: V

Chromium

• Periodic Element

• Atomic Number: 24

• Symbol: Cr

Manganese

• Periodic Element

• Atomic Number: 25

• Symbol: Mn

Iron

• Periodic Element

• Atomic Number: 26

• Symbol: Fe

Cobalt

• Periodic Element

• Atomic Number: 27

• Symbol: Co

Nickle

• Periodic Element

• Atomic Number: 28

• Symbol: Ni

Copper

• Periodic Element

• Atomic Number: 29

• Symbol: Cu

Zinc

• Periodic Element

• Atomic Number: 30

• Symbol: Zn

Gallium

• Periodic Element

• Atomic Number: 31

• Symbol: Ga

Germanium

• Periodic Element

• Atomic Number: 32

• Symbol: Ge

Arsenic

• Periodic Element

• Atomic Number: 33

• Symbol: As

Selenium

• Periodic Element

• Atomic Number: 34

• Symbol: Se

Bromine

• Periodic Element

• Atomic Number: 35

• Symbol: Br

Krypton

• Periodic Element

• Atomic Number: 36

• Symbol: Kr