IB Chem HL/SL Unit II

synthesis reaction

2 or more substances combine to make something more complex

decomposition reaction

a complex substance breaks down into smaller products

combustion

fuel (CxHy) reacts w/O2 to produce CO2, H2O, and heat

Single Replacement

one element replaces another in a reaction

Double Replacement

2 elements switch places in a reaction

Group 1 metals lose electrons easily because…

they lose electrons easily

Group I metals

Li, Na, K, Rb, Cs, Fr

metalic character

how much a metal acts like a metal

Ionization energy

the energy needed to remove an electron from an atom or molecule

High ionization energy =

low metalic character

Electron Affinity

the tendency of an atom to gain electrons

X(g)+e- —> X-(g)

exothermic 

releases energy and product becomes more stable

Nucleus is + and elctrons are -

so there is a natural pull

Period 3 oxides

Na2O, MgO, Al2O3, SiO2, P4O10, SO2, Cl2O7

Characteristics of Na2O

ionic, basic

Al2O3

ionic

MgO

ionic, basic

SiO2

covalent

P4O6 or P4O10

covalent, acidic

SO2 or SO3

covalent, acidic

Cl2O

covalent

Cl2O7

covalent, acidic

metals are typically

ionic, basic

nonmetals are typically

covalent, acidic

Oxidation state of oxygen

2

oxidation state

charge of an element with O

polyatomic ions

bound covalently but have a -1 charge

hydrogens charge is always

1+

Organic Compound

any carbon containing compound

Wohler Synthesis

made urea inorganically

empirical formula

simplest whole # ratio of atoms (ex: H4O2 → H2O)

molecular formula

actual # of atoms

structural formula

visual representation of how atoms are bonded together

full structural formula

shows ALL atoms and bonds

condensed structural formula

shows how atoms are joined but not all bonds

skeletal formula

shows just the bonds in the carbon skeleton and any groups joined

stereochemical formula

shows relative positions in 3D space

homologous series

same functional group increased by an ethyl group

functional group

an atom or group of atoms that determine behavior and characteristics

saturated hydrocarbons

compounds with a hydrogen deficiency of 0

Alkene

An unsaturated hydrocarbon with a double bond on any carbon

alkynes

An unsaturated hydrocarbon with a triple bond on any carbon

meth

1

eth

2

prop

3

but

4

pent

5

hex

6

hept

7

oct

8

non

9

deca

10

alcohol suffix

ol

alcohol functional group

OH

aldehyde suffix

al

aldehyde functional group

alkanal

ketone suffix

one

ketone/carboxylic acid

carbonyl group

carboxylic acid suffix

oic acid

naming ethers

1. Identify the longest carbon chain- normal alkane

2. smaller alkyl group-alkoxy substituent

   1. ex: methoxy ethane

naming esters

1. Identify/name alkyl group

2. Identify/name parent carboxylic acid

3. change suffix to oate

   1. ex: ethyl methanoate

primary alcohol

A primary alcohol is defined as an alcohol in which the hydroxy group (-OH) is bonded to a primary carbon atom,

secondary alcohol

an organic compound where the hydroxyl (–OH) group is attached to a carbon atom that is bonded to two other carbon atoms

tertiary alcohol

an organic compound where the hydroxyl (-OH) group is bonded to a carbon atom that is itself connected to three other carbon atoms

Structural Isomers

molecules with the same molecular formula but different connectivity of atoms

functional isomers

molecules w/ the same formula but different functional group

acids

a substance that produces H+ ions in solution

Base

a substance that reacts w/acids

Alkalis

a water soluble base

all alkalis are bases but

not all bases are alkalis

Bronsted Lowry acid

a substance that is a proton donor in the forward reaction

Bronsted Lowry Base

a proton acceptor on forward reaction

binary acids

hydro-prefix-acid

Hydroxide formula

OH-

hydroxide conjugates

water, H2O

Nitrate formula

NO-

Nitrate conjugates

nitric acid HNO3

carbonate formula

(CO3)-2

sulfate formula

(SO4)2-

sulfate conjugates

sulfuric acid, H2SO4

Phosphate formula

(PO4)-3

Phosphate conjugates

phosphoric acid, H3PO4