Compounds Formulae and Equations 2.1.2 Flashcards
What is the overall charge of an atom
0
What is an ion
An atom (or group of covalently bonded atoms) has either a positive or negative charge, where number of electrons is different to number of protons, because electrons have been lost or gained
What is a molecule
2 or more (non-metal) atoms covalently bonded (not ionically bonded) with no overall charge
What is an element
A substance containing only one type of atom with the same number of protons in the nucleus
What is a compound
Contains 2 or more types of elements chemically combined in a fixed proportion
What is the charge on a proton
+1
What is the charge on a neutron
0
What is the charge on an electron
-1
How is a negative ion formed
An atom (or group of covalently bonded atoms) gains electrons
How is a positive ion formed
An atom (or group of covalently bonded atoms) loses electrons
What is an ionic bond
Ions held together by the electrostatic force of attraction between positive and negative ions
What charge is usually on a metal ion
Positive
What charge is usually on a non-metal ion
Negative
What ending do you use on the name of a non metal ion which contains only one element
-ide
What are the formula of the 7 key ions :ammonium ,silver, zinc, nitrate, sulfate, carbonate, hydroxide
Ammonium= NH4 plus
Silver=Ag plus
Zinc=Zn 2 plus
Nitrate=NO3 minus
Sulphate=SO4 2 minus
Carbonate=CO3 2 minus
Hydroxide= OH minus
what are the formula of these molecules: ammonia, methane, chlorine, bromine, hydrogen
Ammonia=NH3
Methane= CH4
Chlorine=Cl2
Bromine= Br2
Hydrogen=H2
what is a covalent bond
Strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the two bonded atoms
What type of bonding is usually between a metal and a non-metal
Ionic bonding
What type of bonding occurs between 2 non-metals
Covalent bonding
What is an atom
The smallest particle of an element that gives it its chemical properties. It contains a nucleus with protons (1+ charge) and neutrons ( 0 charge) surrounded by shells of electrons with a 1- charge
What is a group on the periodic table and what does it tell us
A vertical column in the periodic table, all the elements in the same group have the same number of outer shell electrons in an atom
What is an atomic number
The number of protons in the nucleus of an atom
What is the mass number
The sum of protons and neutrons in the nucleus
What is a cation
A positively charged ion with fewer electrons than protons (as it has lost electrons to another species)
What is an anion
A negatively charged ion with more electrons than protons (as it has gained electrons from another species)
What is a polyatomic ion
An ion containing more than one atom
What are lone pairs
An outer shell pair of electrons that is not involved in chemical bonding
What is ionic bonding
Strong electrostatic force of attraction between positive and negative ions
What is empirical formula
Shows the simplest whole number ratio of atoms of each element in a compound. (Formula of ionic compounds are always empirical formula)
What is molecular formula
Shows the actual number and type of atoms of each element in a molecule
What is dative covalent bond
A covalent bond in which the shared pair of electrons has been provided by one of the bonding atoms only
What is metallic bonding
Strong electrostatic force of attraction between the cations (positive ions) and delocalized electrons
Define acid
A species that releases/donates a proton ( H+ ions ) in aqueous solution
Define base
A species that accepts a proton ( H+ ions ) in aqueous solution, a compound that neutralizes the acid to form a salt
What is salt
The ionic compound formed from a reaction between an acid and a base
What are spectator ions
Spectator ions are ions that are
* Not changing state
* Not changing oxidation number
during a chemical reaction
What does a metal element do to become a cation
A metal element loses electrons from its outer shell to form a positive ion called a cation
Elements in group 1 loose how many electrons and what charge do they have and become as a result
Elements in group 1 loose 1 electron to form 1 + ion
Elements in group 2 loose how many electrons and what charge do they have and become as a result
Elements in group 2 loose 2 electrons from their outer shell to form a 2+ ion
Elements in group 3 loose how many electrons and what charge do they have and become as a result
Elements in group 3 loose 3 electrons from their outer shell to form a 3+ ion
What charge do the ions have from each group
Group 1
Group 2
Group 3
Group 1 = 1+
Group 2 = 2+
Group 3 =3+
Metal elements in group 4 usually loose how many electrons and give examples
Metal elements in group 4 usually only loose 2 electrons to form a 2+ ion
e.g. Pb 2plus and Sn 2 plus
How many electrons are lost from transition metals
Transition elements can loose different number of electrons to form different positive ions
How do you know how many electrons a transition metal has lost e.g. Iron (II)
The number of electrons lost is written in Roman Numerals in brackets after the metal
E.g. Iron (II) would be Fe 2 plus
Iron (III) would be Fe 3 plus
Is hydrogen a metal or non-metal
Non-metal
What charge does a non–metal form
A non-metal element gains electrons in its outer shell to form negative ions called anions
Elements in group 7 gain how many electrons and what charge do they have and become as a result
Elements in group 7 gain 1 electron to form a 1- ion e.g. Cl-
Elements in group 6 gain how many electrons and what charge do they have and become as a result
Elements in group 6 gain 2 electrons to form a 2- ion
e.g. O 2 minus
Elements in group 5 gain how many electrons and what charge do they have and become as a result
Elements in group 5 gain 3 electrons to form a 3 - ion
e.g. N 3 minus
What charge do the ions have from each group
Group 5
Group 6
Group 7
Group 5 = 3 minus
Group 6= 2 minus
Group 7= 1 minus
How do you determine the name of a cation
Name of metal (+ Roman numbers to show charge if transition metal)
How do you determine the name of the anion
Name of non-metal- but change ending to -ide
How is a giant ionic lattice formed
Oppositely charged ions attract each other and form a giant ionic lattice- cation + anion
In a giant ionic lattice what are bigger the cations or the anions
Negative anions are bigger than positive cations in a giant ionic lattice
What is the overall charge in an ionic compound
There is no overall charge in an ionic compound
True or False
The amount of positive charge must equal to the amount of negative charge in an ionic compound
True hence there is no overall charge on an ionic compound
What do ionic solids show
Formula shows the ratio of cations (+) to anions (-) and no charges are shown in the formula
Multiples of ions are represented by what
A subscript number after the ion
Ions containing more than one element need what
Brackets
Positive ions are usually what and Negative ions are usually what
Positive ions are usually metals and Negative ions are usually non-metals
In covalent bonds, electrons are…
Shared between the atoms (there are no ions)
In a covalent bond there are no what
Ions
Covalently bonded molecules can be
single or a compound containing different elements
What are diatomic molecules
Molecule contains 2 atoms
Group 7 and gaseous elements are diatomic molecules
Salt containing a nitrate ion would result in a solution or precipitate?
All solution
Salt containing a Sulphate ion would result in a solution or precipitate?
Solution except silver, barium, strontium, calcium and lead
Salt containing a Halide (chloride, bromide etc.) ion would result in a solution or precipitate?
Solutions except silver, lead and mercury
Salt containing a carbonate ion would result in a solution or precipitate?
Precipitate except sodium, potassium and ammonium
Salt containing a hydroxide OH- ion would result in a solution or precipitate?
Most are insoluble except group 1+ ammonium which are soluble
How do you work out the formula of a written equation from its ionic charge?
e.g. Lithium Sulphate
1) Identify formula by identifying ionic charge
Lithium-group 1= 1+ charge= Li+
Sulphate= 2- charge = SO4 2 minus
2) Combine ions together to get a neutral compound by crossing method
Li+ and SO4 2 minus
Li2 SO4
Look in chem book if still not understood
Why do we write ionic equations
To show key changes in a reaction
What do ionic equations show and what do they not show
Show= ions that are reacting
Do not show= spectator ions
Practice balancing equations on sheet- starter quiz 10 marks
Should be in folder with the rest of starter quizzes- its the one with gill that i got 4 out of 10 on
Write and balance equation sheet in 15 minutes
Should be in chem folder with the rest of starter quizzes sheets
Hydrogen
H2
Hydride
H minus
Sodium
Na plus
Potassium
K plus
Calcium
Ca 2 plus
Magnesium
Mg 2 plus
Carbonate
CO3 2 minus
Hydrogen Carbonate
HCO3 minus
Ammonium
NH4 plus
Nitrate
NO3 minus
Nitride
N 3 minus
Phosphate
PO4 3 MINUS
Phosphide
P 3 minus
Hydroxide
OH minus
Oxide
O 2 minus
Sulphate
SO4 2 minus
Sulfide
S 2 minus
Hydrogen Sulphate
HSO4 minus
Fluoride
Chloride
F minus
Cl minus
Bromide
Iodide
Br minus
I minus
D block: Transition metals
Iron (II)
Lead (II)
Silver
Copper (I)
diChromate (VI)
Manganate (VII)
Iron (II)= Fe 2plus
Lead (II)= Pb 2 plus
Silver = Ag plus
Copper (I)= Cu plus
diChromate (VI)= Cr2O7 2 minus
Manganate (VII)= MnO4
D block: Transition metals
Zinc
Iron (III)
Lead (IV)
Copper (II)
Chromium (III)
Manganese (II)
Zinc = Zn 2 plus
Iron (III) = Fe 3 plus
Lead (IV) = Pb 4 plus
Copper (II) = Cu 2 plus
Chromium (III) = Cr 3 plus
Manganese (II) = Mn 2 plus
Polyatomic ions have atoms joined together by covalent bonds but have…
Lost or gained electrons overall
Name 3 gaseous elements that are diatomic molecules
Hydrogen= H2
Oxygen= O2
Nitrogen= N2
Name 4 group 7 elements that are diatomic molecules
Fluorine= F2
Chlorine= Cl2
Bromine= Br2
Iodine= I2
Name 5 covalently bonded compounds
Carbon dioxide
Methane
Water
Carbon monoxide
Ammonia
Carbon dioxide
CO2
Carbon monoxide
CO
Methane
CH4
Water
H2O
Ammonia
NH3
Name the following compounds
NaCl
ZnSO4
PbO
CuCO3
CaCl2
Al(OH)3
NaHCO3
Zn(NO3)2
Sodium Chloride
Zinc Sulphate
Lead Oxide
Copper Carbonate (II)
Calcium Chloride
Aluminum Hydroxide
Sodium Hydrogen carbonate
Zinc Nitrate
Write out the formula for the following:
1) Copper Oxide
2) Lead Sulphate
3) Calcium Oxide
4) Potassium Chloride
5) Iron (II) Hydroxide
6) Ammonium Chloride
1) CuO
2)PbSO4
3)CaO
4)KCl
5) Fe(OH)2
6) NH4Cl
Do Task 2 in Compounds, Formula and Equations booklet
Really good practice
Do Task 4 in Compounds, Formula and Equations booklet
Booklet should be in Chem folder but answers are in Orange Chem book
Do the questions after Task 4, the exam style practice in Compounds, Formula and Equations booklet
Booklet should be in Chem folder but answers are in Orange Chem book
Do Task 5 Questions 3a, 3b, 3c, and 3d in Compounds, Formula and Equations booklet
Booklet should be in Chem folder but answers are in Orange Chem book, if not there then look online in Gills resources
Do Task 6 in Compounds, Formula and Equations Booklet
Look on Gills resources for Questions and then look at my booklet for answers, do this on a white board and try do as many questions as possible in 15 minutes
Do Task 7 and answer questions 1-5 in Compounds, Formula and Equations Booklet
Answers are on Gills resources
https://edukedstac-my.sharepoint.com/:b:/g/personal/ke1448_kedst_ac_uk/EazYW8QdDXxFi3RP_Lf7Jp4BgO4usGAB-6xscxYuupkw_g?e=UUIfdf
Do Task 7 and answer questions 5-10, in Compounds, Formula and Equations booklet
Answers are on Gills resources
https://edukedstac-my.sharepoint.com/:b:/g/personal/ke1448_kedst_ac_uk/EazYW8QdDXxFi3RP_Lf7Jp4BgO4usGAB-6xscxYuupkw_g?e=UUIfdf
In Compounds Formula and Equations Booklet do Kerboodle Summary questions and the table underneath, its on the last page
Answers are on kerboodle textbook page 273, under the sub-heading 2.3
https://www.kerboodle.com/api/courses/14989/interactives/102929.html
Do All practice questions on page 19 of Kerboodle Chemistry year 1 AS book
https://www.kerboodle.com/system/images/W1siZiIsIjIwMTcvMDUvMjIvMTIvNTEvNDYvODU2L294b19BQ2hlQV8wMnV1X3NiMDFfeHhhYW5uLnBkZiJdXQ/oxo_ACheA_02uu_sb01_xxaann.pdf
Do Questions 1, 2, and 3 in the C3 Booklet of Compounds, Formulae and Equations
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Do Questions 4, 5 and 6 in the C3 Booklet of Compounds, Formulae and Equations
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Do Questions 7, 8 and 9 in the C3 Booklet of Compounds, Formulae and Equations
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Do Questions 10, 11 and 12 in the C3 Booklet of Compounds, Formulae and Equations
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Click on the first QR code on compounds formulae and equations booklet and name all ions
Do 2nd QR code on Compounds Formulae and Equations booklet on ions
Do 3rd and 4th QR code on Compounds, Formulae and Compounds Booklet
Do Task 5 question 2 A and B in Compounds, Formula and Equations booklet
Do Task 5 question 4 A and B in Compounds, Formula and Equations booklet
Do practice balancing equations sheet the one i got 4/10 on
Should be with the rest of the compounds formulae and equation booklet. its got an orange highlighter mark by my name in the top left hand corner
Do the test or starter quiz that says Task 1 Writing and naming ions
Should be with the rest of the compounds formulae and equations booklet its got purple writing on and i got 13/20 on it. Re attempt in 10 minutes, start by seeing how long it takes then work backwards but write down the time, do not attempt right after wait for next time so you can beat already set limit
Complete questions 1-5 on gap task: Atomic & Electron Structure, Isotopes and Formulae Test
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Complete questions 6-10 on gap task: Atomic & Electron Structure, Isotopes and Formulae Test
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Complete questions 11 on gap task: Atomic & Electron Structure, Isotopes and Formulae Test
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Complete extension question 1 on gap task: Atomic & Electron Structure, Isotopes and Formulae Test
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Complete Atomic & Electron Structure, Isotopes and Formulae Test
Mark each question as you go, should be with the rest of the things in chem folder
Number 1 in Roman Numerals
I
Number 2 in Roman Numerals
II
Number 3 in Roman Numerals
III
Number 4 in Roman Numerals
IV
Number 5 in Roman Numerals
V
Number 6 in Roman Numerals
VI
Number 7 in Roman Numerals
VII
Number 8 in Roman Numerals
VIII
Number 9 in Roman Numerals
IX
Number 10 in Roman Numerals
X
Make flashcards on every single polyatomic ion on the front page of Compounds, formulae and Equations booklet
Do exam practice from physics and maths tutor and make notes and flashcards of questions got wrong
