Grade 11 Chem Exam

Dobereiner

law of triads

Newlands

law of octaves

Mendeleev

arranged elements by atomic mass

What elements are liquid at SATP?

Mercury and Bromine

John Dalton

• billiard ball model

• law of conservation mass ,definite proportions and constant composition

• atomic theory

JJ Thompson

• plum pudding model

• cathode raw tube experiment

• discovered electrons

Nagakoa

Saturnia

Rutherford

• nuclear model

• gold foil experiment

• noticed a small dense positive center

Bohr

• planetary model

• discovered energy levels

Chadwick

• Alpha particles experiment

• discovered neutrons

atomic number

number of protons

nuclear charge

number of protons

mass number

number of protons and neutrons

isotope

a change in the number of neutrons

atomic mass

the relative mass of an atoms when C-12 = 12u

what are the 3 diagrams used to represent elements?

1. bohr-rutherford diagram

2. electron arrangement diagram

3. electron dot diagram

Isotopic abundance

the percentage abundance of an isotope

average atomic mass

the average of the atomic masses of the isotopes of an element

atomic radius

the distance between the nucleus and the outermost electron

Ionization enegery

the amount of energy requires to remove and electron in the gaseous state

electronegativity

the ability of an atom to attract electrons when bonded

Electron affinity

amount of energy released when an electron attatches to a neutral atom

shielding effect

the repulsion felt by the valence electrons from the inner electrons

effective nuclear charge

the net attraction felt by the valence electrons

successive ionization energy

shows the change in ionization energy with each electron being removed

ionic compound properties

solid, high melting and boiling points, mostly white, dissolve, conductive, hard, brittle

isoelectronic

when an ion with a stable octet resembles its nearest noble gas

Lower charge ending for multivalent metals

ous

Higher charge ending for multivalent metals

ic

Classical root for Iron

Ferr

Classical root for Copper

Coupr

Classical root for Tin

Stann

Classical root for Lead

Plumb

Classical root for Antimony

Stibn

Classical root for Cobalt

Cobalt

Classical root for Gold

Aur

Classical root for Mercury

Mercury

Modifying the number of oxygens in polyatomic ions

1. one less: ____ite

2. two less: hypo_____ite

3. one more: per____ate

Adding an extra H to a polyatomic ion

“bi______” or “hydrogen ____”

Hydrate

an ionic compound with water

Notation for a hydrate

“__hydrate”

_____-#H2O

Properties of molecular compounds

solid liquid or gas, dissolve well or not at all, non conductive

Bonding pairs

te electrons that are between elements

lone pairs

electrons that aren’t bonded, only attatched to one element

1

mono

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

10

deca

H2O

Water

NH3

Ammonia

CH4

Methane

C3H8

Propane

C6H12O6

Glucose

C12H22O11

Sucrose

C2H5OH

Ethanol

Diatomic molecules

H, O, F, Br, I, N, Cl

naming for acids

IUPAC: Aqueous Hydrogen ____

Classical: Hydro____ic acid

Naming for basses

Aqueous _____ hydroxide

Pure covalent bond

Electrons are shared equally, Delta EN < 0.40

Polar covalent bond

Electrons are not shared equally, 0.40 < delta EN < 1.70

Ionic bond

electrons are transferred, delta EN > 1.70

Combustion reaction

a reaction containing oxygen that produces oxides and releases energy

Exothermic reaction

a reaction with a NET release of energy

Cobalt II chloride paper test

tests for water, turns pink

Limewater test

Tests for carbon dioxide, turns cloudy

Flaming splint test

test for hydrogen

Glowing splint test

tests for oxygen

Properties of a complete combustion reaction

blue flame is produced, products are CO2, H2O and energy

Properties of an incomplete combustion reaction

Orange flame is produced, products are CO2, CO, C, H2O and energy

Synthesis

the combination of two elements or compounds to form a new compound

decomposition

the separation of a compound into simpler elements of compounds

single displacement

when one element replaces another in a compound

Double displacement reaction

when two aqueous compounds react to form a precipitate or a gas

Molar mass

the mass of one mole of a substance

Atomic mass

the mass of an atom

molecular mass

the ass of a molecular compound

Formula mass

the mass of an ionic compound

A mole

a quantity of a substance that contains 6.02×10²3 number of units

percentage composition

the quantity of each element that makes up a compound

percentage composition by mass

the mass of an element in a compound

Empirical formula

the simplest form of a substance, many compounds are able to have the same EF

Molecular formula

The actual formula of a substance containing the actual numbers of each element

Stoichiometry

compares the relationship between the amount of reactants and products

limiting reagent

the reactant that is used up fully and limits the amount of product formed

excess reagent

th reactant that is not used up completely

theoretical yield

the maximum amount of a product that could potentially form

actual yield

The amount of product that actually forms in a chemical reaction

Percentage yield

the actual yield expressed as a percent of the theoretical yield

Flint water crisis

lead pipes oxidized due to low pH, forminb Pb ions

Solvent

the substance dissolving the solute

solute

the substance being dissolved

dissociation

when water separates ionic compounds by surrounding its ions

dissolving

LIKE DISSOLVES LIKE

asymmetrical

polar, dissolves