Grade 11 Chemistry Notes
Chapter One
Chemistry – the science of composition, structure, properties, and reactions of matter.
Collect Data, Hypothesize, test hypothesis, modify hypothesis.
Matter – anything that occupies space and has mass
Chapter Two
Volume – 1L
1mL – 1cm^3
For unit conversion – cross out units to get rid off like a fraction
Density = mass/volume = g/mL
Chapter Three
Elements are fundamental substances that cannot further be broken to smaller substances
Metals are less active in combining with other elements, metals often mix with other metals to form
homogeneous solids called alloys
Non-metals form molecular compounds
Metalloids are intermediate properties
Diatomic Molecules exist as pairs. Form a 7 on periodic table
Compounds & Formulas – can be decomposed into smaller substances, always whole numbers
Molecule – union of two or more atoms, smallest composition
Ion – positive or negative net charge of atom(s) – help by electrostatic force
Molecular Compound – held by covalent bonds,
Ionic Compound – help by electrostatic force,
Compounds can be identified through characteristic properties
Formulas of Compounds – shows symbols and ratios of atoms
Tells us the reactants and products
When more than one group of atoms occurs as a unit, brackets around the group. Subscript to right or
brackets
Compounds Composition – contain same elements in same proportions
LoDC: Compounds contain two or more elements combined in definite proportion by mass:
8g of O present in 1g of H in H20. 16g of O present in 1g of H in H2O2. 2:1 ratio if oxygen in hydrogen
peroxide to water
LoMP: Atoms of two or more elements can combine in different ratios to produce more than one
compound: CuCl2, CuCl
Chapter Four
Properties of Substances
Recognize substances by physical and chemical properties.
EX. Chlorine: gas at room temp, 2.4x heavier than air, yellow color. Chemically, will not burn but support
combustion of other substances. Used as a bleaching agent, disinfectant.
Physical & Chemical change – size, shape, density. (same composition) - change in composition and
substance is chemical change. Cannot be reversed.
,Ex. Copper when burnt, oxidises, making copper(II) oxide after oxygen exposure.
Decomposition can be achieved by electrolysis.
Delta represents heat (thermal energy) – flow on E due to temp difference
Solving Problems
Read – find knowns and unknowns
Plan – determine principles, units necessary
Calculate – preform math necessary
Check – rationale
Energy – mechanical, chemical, nuclear, radiant, light, heat.
Potential E - stored energy due to relative position or height. Ex. Gasoline hold Ep until it burns then
releases the Ep
Kinetic E – energy due to motion.
Mechanical E can turn to electrical E with 90% efficiency.
Energy in Chemical Changes – all energy essential to life is produced by chemical change
Also, energy is needed to cause chemical changes.
When H is used as fuel, E is released, lowering potential energy.
Conservation of Energy
Energy can change forms or substances but can not be lost.
Initial Energy = Final Energy
Heat: Quantitative Measurement
Energies SI unit (kg*m2/s2) Joules. 4.184J = 1 calorie – change 1g of water temp by 1 degree. cal – joule
– divide by 4.184
Use kilo prefix for calories and joules in chemical processes.
Temp – measure of heat.
Heat – flow of energy due to change in temp/ temp difference
Specific heat – quantity of heat needed to change 1g of a substance by 1 degree
Energy in Real World
Hydrocarbon compounds are compounds containing different mixes of Hydrogen and Carbon.
Hydrocarbon makes up petroleum which we use as fuel and gasoline for cars and machinery and much
more.
Chapter Five
Early Atomic Theory & Structure
Elements are minute atoms
Atoms of same elements are alike in size and mass
Atoms of different elements have different masses and sizes
Chemical compounds are formed by union of two or more atoms of different elements
Atoms combine to form compounds in simple numerical ratios, 1:1, 2:1, 3:1
Atoms of two elements may combine in different ratios to form different compounds
Electric Charge – radius of hydrogen – 5.29x10^-11m
Induction or Conduction, force is inversely proportional to square of radius
Faraday called ions because of attraction to electrodes
Nuclear Atom
Small with electron orbiting in clouds with DE Broglie wavelength
Electron clouds.
Mass of atom is its nucleus
, Isotopes
Same atomic number but different atomic mass. Different amount of neutrons
Mass number – p + n
Atomic Mass
C-12 is reference isotope. 1/12th
Atomic mass is the average of all the found isotopes of the element, to find which isotope Is most
abundant
Atomic mass of an element is the average relative mass of the isotopes of that element compares to
carbon-12
Chapter Six
Common Systematic names
# of elements present
1 - element
2 – Binary Compound
3+ - polyatomic compound
Elements & Ions
When atom loses an electron or gains you add a plus or minus
Ions can be formed by adding or removing an electron
To name an anion consisting of one element add -ide ion
Ions form when metals and non-metals combine
1A,2A,3A,4A,5A,6A,7A were 1-3 are positive and 5-7 are negative ions
Transition metals form cations with positive charges
All metals loose electrons to form positive ions
Non-metals form anions by electron gain
Writing Formulas from names of Ionic compounds
Chemical compound must have net charge of zero
If it contains ions the charge must balance to zero
Find lowest common multiple – then balance to zero with maths
Binary Compounds
Containing a metal with one type of cation
Metal + non-metal = binary ionic compound
Metal loses one or more e- and non-metal gains e-
Cation before anion in formula
Write cation then anion stem and -ide
Binary Ionic Compounds w/ a metal able to form two or more cations
For cation charge put roman numeral after metal name
If a compound has two or more negative ions with a -1 charge, deduce that the metal has a +charge
Rules for naming – write cation, write charge as roman numerals, add stem of anion + ide
Classically in nomenclature, metallic ions with two cations, the name of the metal is modified with
suffixes -ous (lower charge) & -ic (higher charge)
Binary Compounds with Two Non-Metals
Follow order for naming compounds – Si, B, P, H, C, S, I, C, Br, N, Cl, O, F
Name of second element retains -ide
Latin or Greek prefix attached to name of each element to indicate number of atoms of that element in
a molecule
Mono – 1, di – 2, tri – 3, tetra – 4, penta – 5, hexa – 6, hepta – 7, octa – 8, nona – 9, deca – 10
Chapter One
Chemistry – the science of composition, structure, properties, and reactions of matter.
Collect Data, Hypothesize, test hypothesis, modify hypothesis.
Matter – anything that occupies space and has mass
Chapter Two
Volume – 1L
1mL – 1cm^3
For unit conversion – cross out units to get rid off like a fraction
Density = mass/volume = g/mL
Chapter Three
Elements are fundamental substances that cannot further be broken to smaller substances
Metals are less active in combining with other elements, metals often mix with other metals to form
homogeneous solids called alloys
Non-metals form molecular compounds
Metalloids are intermediate properties
Diatomic Molecules exist as pairs. Form a 7 on periodic table
Compounds & Formulas – can be decomposed into smaller substances, always whole numbers
Molecule – union of two or more atoms, smallest composition
Ion – positive or negative net charge of atom(s) – help by electrostatic force
Molecular Compound – held by covalent bonds,
Ionic Compound – help by electrostatic force,
Compounds can be identified through characteristic properties
Formulas of Compounds – shows symbols and ratios of atoms
Tells us the reactants and products
When more than one group of atoms occurs as a unit, brackets around the group. Subscript to right or
brackets
Compounds Composition – contain same elements in same proportions
LoDC: Compounds contain two or more elements combined in definite proportion by mass:
8g of O present in 1g of H in H20. 16g of O present in 1g of H in H2O2. 2:1 ratio if oxygen in hydrogen
peroxide to water
LoMP: Atoms of two or more elements can combine in different ratios to produce more than one
compound: CuCl2, CuCl
Chapter Four
Properties of Substances
Recognize substances by physical and chemical properties.
EX. Chlorine: gas at room temp, 2.4x heavier than air, yellow color. Chemically, will not burn but support
combustion of other substances. Used as a bleaching agent, disinfectant.
Physical & Chemical change – size, shape, density. (same composition) - change in composition and
substance is chemical change. Cannot be reversed.
,Ex. Copper when burnt, oxidises, making copper(II) oxide after oxygen exposure.
Decomposition can be achieved by electrolysis.
Delta represents heat (thermal energy) – flow on E due to temp difference
Solving Problems
Read – find knowns and unknowns
Plan – determine principles, units necessary
Calculate – preform math necessary
Check – rationale
Energy – mechanical, chemical, nuclear, radiant, light, heat.
Potential E - stored energy due to relative position or height. Ex. Gasoline hold Ep until it burns then
releases the Ep
Kinetic E – energy due to motion.
Mechanical E can turn to electrical E with 90% efficiency.
Energy in Chemical Changes – all energy essential to life is produced by chemical change
Also, energy is needed to cause chemical changes.
When H is used as fuel, E is released, lowering potential energy.
Conservation of Energy
Energy can change forms or substances but can not be lost.
Initial Energy = Final Energy
Heat: Quantitative Measurement
Energies SI unit (kg*m2/s2) Joules. 4.184J = 1 calorie – change 1g of water temp by 1 degree. cal – joule
– divide by 4.184
Use kilo prefix for calories and joules in chemical processes.
Temp – measure of heat.
Heat – flow of energy due to change in temp/ temp difference
Specific heat – quantity of heat needed to change 1g of a substance by 1 degree
Energy in Real World
Hydrocarbon compounds are compounds containing different mixes of Hydrogen and Carbon.
Hydrocarbon makes up petroleum which we use as fuel and gasoline for cars and machinery and much
more.
Chapter Five
Early Atomic Theory & Structure
Elements are minute atoms
Atoms of same elements are alike in size and mass
Atoms of different elements have different masses and sizes
Chemical compounds are formed by union of two or more atoms of different elements
Atoms combine to form compounds in simple numerical ratios, 1:1, 2:1, 3:1
Atoms of two elements may combine in different ratios to form different compounds
Electric Charge – radius of hydrogen – 5.29x10^-11m
Induction or Conduction, force is inversely proportional to square of radius
Faraday called ions because of attraction to electrodes
Nuclear Atom
Small with electron orbiting in clouds with DE Broglie wavelength
Electron clouds.
Mass of atom is its nucleus
, Isotopes
Same atomic number but different atomic mass. Different amount of neutrons
Mass number – p + n
Atomic Mass
C-12 is reference isotope. 1/12th
Atomic mass is the average of all the found isotopes of the element, to find which isotope Is most
abundant
Atomic mass of an element is the average relative mass of the isotopes of that element compares to
carbon-12
Chapter Six
Common Systematic names
# of elements present
1 - element
2 – Binary Compound
3+ - polyatomic compound
Elements & Ions
When atom loses an electron or gains you add a plus or minus
Ions can be formed by adding or removing an electron
To name an anion consisting of one element add -ide ion
Ions form when metals and non-metals combine
1A,2A,3A,4A,5A,6A,7A were 1-3 are positive and 5-7 are negative ions
Transition metals form cations with positive charges
All metals loose electrons to form positive ions
Non-metals form anions by electron gain
Writing Formulas from names of Ionic compounds
Chemical compound must have net charge of zero
If it contains ions the charge must balance to zero
Find lowest common multiple – then balance to zero with maths
Binary Compounds
Containing a metal with one type of cation
Metal + non-metal = binary ionic compound
Metal loses one or more e- and non-metal gains e-
Cation before anion in formula
Write cation then anion stem and -ide
Binary Ionic Compounds w/ a metal able to form two or more cations
For cation charge put roman numeral after metal name
If a compound has two or more negative ions with a -1 charge, deduce that the metal has a +charge
Rules for naming – write cation, write charge as roman numerals, add stem of anion + ide
Classically in nomenclature, metallic ions with two cations, the name of the metal is modified with
suffixes -ous (lower charge) & -ic (higher charge)
Binary Compounds with Two Non-Metals
Follow order for naming compounds – Si, B, P, H, C, S, I, C, Br, N, Cl, O, F
Name of second element retains -ide
Latin or Greek prefix attached to name of each element to indicate number of atoms of that element in
a molecule
Mono – 1, di – 2, tri – 3, tetra – 4, penta – 5, hexa – 6, hepta – 7, octa – 8, nona – 9, deca – 10
