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Chemistry Unit 1 Grade 11
Grade 10 Knowledge
Polytomic Ions
Carbonate
CO32-
Hydroxide
OH-
Phosphate
PO43-
Fluorate
FO3-
Bromate
BrO3-
Ammonium
NH4+
Permanganate
MnO42-
Nitrate
NO3-
Sulfate
SO42-
Chlorate
ClO3-
HOFBrINCl
mnemonic device used in Chemistry to remember the diatomic molecules, which are molecules consisting of two atoms
Hydrogen, Oxygen , Fluoride, Bromine, Iodine, Nitride, Chloride
Atomic Radii
Atomic Radii is the size of an atom, similar to the word “Radius”, It’s chemistry’s unit of measurement to find the radius of an atom.
Atomic Radii Trend
On the Periodic Table, there’s a trend that shows that any element that progresses furthest to the bottom left of the periodic table will have a larger atomic radius than those on the top right, being the largest. The Alkali Metals are a perfect example as they gain an additional energy shell than the previous element and have 1 electron on their outer ring, leaving with the results of a lower force of attraction.
This rule isn’t applicable to every SINGLE element but for the most part, it is accurate.
Effective Nuclear Charge
Known as “Zeff” or just “Z”, It’s the positive charge of pulling electrons towards the nucleus. To not confuse you, it is completely different from its actual nuclear charge as it’s based on the attraction close to the positively charged nucleus (relying on the amount of protons existing) rather than the amount of electrons it’s attempting to attract to satisfy its valence.
To simplify, It’s determined by the outer shell amount of electrons, representing itself as “Zeff.” To discover this we must set an example, Carbon (C) will be our example. Carbon has a charge of 4+ or - but to answer its effective nuclear charge, we must subtract its inner rings worth of electrons to find our Z. Formula is built off as “Zeff = #protons - #inner electrons.” Giving us the answer that Carbon’s Zeff is 4.
Ionization Energy
It’s the measurement to see the amount of energy required to remove an electron from an isolated atom to acquire a negative or positive charge.
Ionization Energy shown on the Periodic Table
On the Periodic Table, There’s a trend that is shown that any element that is closest to the top right of the periodic table will have the highest amount of ionization energy. Example would be the Noble gases as they are the only elements with a complete valence shell, hence why you almost never see them mixed with other elements as it requires a lot of energy to remove a single electron from its shell.
This rule is not implemented to every SINGLE element but overall accurate to be a trend.
Electron Affinity
A measurement of the attraction between the incoming electron and nucleus. It’s basically the opposite of ionization energy on the periodic table as instead of measuring the amount of energy change after gaining an electron.
Electron affinity Trend/Ionization Energy shown on the Periodic Table
On the Periodic Table, There’s a trend that is shown that any element that is closest to the top right of the periodic table will have the highest amount of ionization energy/Electron Affinity. Example would be the Noble gases as they are the only elements with a complete valence shell, hence why you almost never see them mixed with other elements as it requires a lot of energy to remove/add a single electron from its shell.
This rule is not implemented to every SINGLE element but overall accurate enough to be a trend.
Reactivity (Same trend as Radii)
Metals react by losing electrons and the lower the attraction for outer electrons, the greater reactivity.
Non metals react by gaining electrons
The greater the attraction for outer electrons, the greater the reactivity.
Ionic Bonds
It’s the process of 2 or more atoms transferring its electrons to another atom in order to complete their desired valence shell amount. This bond only happens between a metal and non-metal atom.
Note that an electron transfer will cause a negative charge (Known as anion, an ion that is negatively charged) or positive charge (known as a cation, an ion that is positively charged).
All electrons lost by the metal are gained by the non metal
Properties of ionic substances/compounds
Crystal lattice when solid at room temperature
High melting/ boiling points
Hard but very brittle in water
Covalent bonding
A bond that happens between a non metal and non metal. Main difference from ionic bonds is that they share electrons rather than transfer their electrons creating a new type of compound which is called “Covalent Compound.”
No ions are formed from the creation of the compounds.
Formula for drawing Lewis Dot Diagram
# of atoms • electron amount +... = total number of electrons
Properties of non-metal substances/compounds
Form molecules that can turn into any state of matter (Solids, liquids, gasses)
Low melting/ boiling points
Multiple Bonds Resonance structures
If you’re not certain where the bonds need to go so you show all possible solutions.
Expanded Valences
Octet rule allows a max of 4 bonds but some allow 8, only for those with an atomic number greater than 10.
VSEPR Geometry
What is VSEPR?
VSEPR stands for valence shell electron pair repulsion and it presents us the idea if electron pairs repel each other whether or not they are in bond pairs or in lone pairs.
Formula for VSEPER is AB#E#
A represents Central Atom
B represents Bonding Electron Pairs
E represents non bonding lone electron pairs
# represents the amount of Bonding electrons there are or lone pairs.
VSEPR Diagrams
There are 5 different types of Diagrams you must remember and their formulas.
Linear Diagram
A straight line
Formula = AB2E0
Grade 10 Knowledge
Polytomic Ions
Carbonate
CO32-
Hydroxide
OH-
Phosphate
PO43-
Fluorate
FO3-
Bromate
BrO3-
Ammonium
NH4+
Permanganate
MnO42-
Nitrate
NO3-
Sulfate
SO42-
Chlorate
ClO3-
HOFBrINCl
mnemonic device used in Chemistry to remember the diatomic molecules, which are molecules consisting of two atoms
Hydrogen, Oxygen , Fluoride, Bromine, Iodine, Nitride, Chloride
Atomic Radii
Atomic Radii is the size of an atom, similar to the word “Radius”, It’s chemistry’s unit of measurement to find the radius of an atom.
Atomic Radii Trend
On the Periodic Table, there’s a trend that shows that any element that progresses furthest to the bottom left of the periodic table will have a larger atomic radius than those on the top right, being the largest. The Alkali Metals are a perfect example as they gain an additional energy shell than the previous element and have 1 electron on their outer ring, leaving with the results of a lower force of attraction.
This rule isn’t applicable to every SINGLE element but for the most part, it is accurate.
Effective Nuclear Charge
Known as “Zeff” or just “Z”, It’s the positive charge of pulling electrons towards the nucleus. To not confuse you, it is completely different from its actual nuclear charge as it’s based on the attraction close to the positively charged nucleus (relying on the amount of protons existing) rather than the amount of electrons it’s attempting to attract to satisfy its valence.
To simplify, It’s determined by the outer shell amount of electrons, representing itself as “Zeff.” To discover this we must set an example, Carbon (C) will be our example. Carbon has a charge of 4+ or - but to answer its effective nuclear charge, we must subtract its inner rings worth of electrons to find our Z. Formula is built off as “Zeff = #protons - #inner electrons.” Giving us the answer that Carbon’s Zeff is 4.
Ionization Energy
It’s the measurement to see the amount of energy required to remove an electron from an isolated atom to acquire a negative or positive charge.
Ionization Energy shown on the Periodic Table
On the Periodic Table, There’s a trend that is shown that any element that is closest to the top right of the periodic table will have the highest amount of ionization energy. Example would be the Noble gases as they are the only elements with a complete valence shell, hence why you almost never see them mixed with other elements as it requires a lot of energy to remove a single electron from its shell.
This rule is not implemented to every SINGLE element but overall accurate to be a trend.
Electron Affinity
A measurement of the attraction between the incoming electron and nucleus. It’s basically the opposite of ionization energy on the periodic table as instead of measuring the amount of energy change after gaining an electron.
Electron affinity Trend/Ionization Energy shown on the Periodic Table
On the Periodic Table, There’s a trend that is shown that any element that is closest to the top right of the periodic table will have the highest amount of ionization energy/Electron Affinity. Example would be the Noble gases as they are the only elements with a complete valence shell, hence why you almost never see them mixed with other elements as it requires a lot of energy to remove/add a single electron from its shell.
This rule is not implemented to every SINGLE element but overall accurate enough to be a trend.
Reactivity (Same trend as Radii)
Metals react by losing electrons and the lower the attraction for outer electrons, the greater reactivity.
Non metals react by gaining electrons
The greater the attraction for outer electrons, the greater the reactivity.
Ionic Bonds
It’s the process of 2 or more atoms transferring its electrons to another atom in order to complete their desired valence shell amount. This bond only happens between a metal and non-metal atom.
Note that an electron transfer will cause a negative charge (Known as anion, an ion that is negatively charged) or positive charge (known as a cation, an ion that is positively charged).
All electrons lost by the metal are gained by the non metal
Properties of ionic substances/compounds
Crystal lattice when solid at room temperature
High melting/ boiling points
Hard but very brittle in water
Covalent bonding
A bond that happens between a non metal and non metal. Main difference from ionic bonds is that they share electrons rather than transfer their electrons creating a new type of compound which is called “Covalent Compound.”
No ions are formed from the creation of the compounds.
Formula for drawing Lewis Dot Diagram
# of atoms • electron amount +... = total number of electrons
Properties of non-metal substances/compounds
Form molecules that can turn into any state of matter (Solids, liquids, gasses)
Low melting/ boiling points
Multiple Bonds Resonance structures
If you’re not certain where the bonds need to go so you show all possible solutions.
Expanded Valences
Octet rule allows a max of 4 bonds but some allow 8, only for those with an atomic number greater than 10.
VSEPR Geometry
What is VSEPR?
VSEPR stands for valence shell electron pair repulsion and it presents us the idea if electron pairs repel each other whether or not they are in bond pairs or in lone pairs.
Formula for VSEPER is AB#E#
A represents Central Atom
B represents Bonding Electron Pairs
E represents non bonding lone electron pairs
# represents the amount of Bonding electrons there are or lone pairs.
VSEPR Diagrams
There are 5 different types of Diagrams you must remember and their formulas.
Linear Diagram
A straight line
Formula = AB2E0
Bent Angular
Bent Angular
NoteStudied by 9 peopleNoteStudied by 7 peopleNoteStudied by 60 peopleNoteStudied by 26 peopleNoteStudied by 629 peopleNoteStudied by 5 people