Chemistry Spm Definition List.docx
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CHEMISTRY SPM DEFINITION LIST 1.
The proton number of an atom is the number of protons in the nucleus of an atom.
2.
The nucleon number of an atom is the sum of the number of protons and neutrons in the atom.
3.
Isotopes are atoms of the same element with same proton number but different nucleon numbers.
4.
Molecular formula of a compound shows the actual number of atoms of each element that are present in a molecule of the compound.
5.
Empirical formula of a compound shows the simplest whole number ratio of atoms of each element present in the compound.
6.
Ionic bond is the chemical bond formed through the transfer of electrons from metal atoms to non-metal atoms to achieve the stable octet electron arrangement.
7.
Ionic compound consist of positive ions and negative ions which are held by strong electrostatic forces of attraction.
8.
Covalent bond is the chemical bond formed through the sharing of electrons between non metal atoms to achieve the stable duplet or octet electron arrangement.
9.
Covalent compound consists of neutral molecules which are held by weak intermolecular forces (Van der Waals).
10.
Electrolytes are substances that can conduct electricity when they are in molten states or aqueous solution and undergo chemical changes. Electrolytes are ionic compounds which contain freely moved ions and thus, they are able to conduct electricity.
11.
Electrolysis is a process whereby compounds in either molten or aqueous state are broken down into their constituent by passing electricity through them.
12.
An acid is a substance which ionises or dissociates in water to produce hydrogen ion, H+.
13.
A base is a substance which ionises or dissociates in water to produce hydroxide ion, OH-.
14.
An alkali is a base which is soluble in water and ionises or dissociates to produce hydroxide ion, OH-.
15.
Monoprotic acid is an acids which ionizes in water to produce 1 mol of H+ ion. Example: Hydrochloric acid – HCl, Nitric acid – HNO3
16.
Diprotic acid is an acid which ionizes in water to produce 2 mol of H+ ion. Example : Sulphuric acid – H2SO4
17.
Strong alkali is an alkali which ionises (dissociates) completely in water to form high concentration of hydroxide ions, OH-.
18.
Weak alkali is an alkali which ionises (dissociates) partially in water to form low concentration of hydroxide ions, OH-.
19.
Strong acid is an acid which ionises (dissociates) completely in water to form high concentration of hydrogen ions, H+.
20.
Weak acid is an acid which ionises (dissociates) partially in water to form low concentration of hydrogen ions, H+.
21.
An alloy is a mixture of two or more elements in a certain composition in which the major component is a metal.
22.
Polymers are a long chain molecule made by joining together lots of smaller repeating molecules called monomers through a process called polymerisation.
23.
Rate of reaction is the speed at which reactants are converted into the products in a chemical reaction OR the change in the quantity of reactants or products per unit time.
24.
Factors Affecting Rate of Reaction Total Surface Area Temperature Concentration Pressure Presence of Catalysts
25.
Catalyst is a substance that can change / speed up the rate of reaction but remains chemically unchanged at the end of the reaction.
26.
Activation Energy, Ea is the minimum energy the colliding particles must have before collision between them can result in chemical reaction.
27.
28.
Compounds Alkanes Alkenes
General formula CnH2n+2 CnH2n, where n = 2, 3 …
Alcohol
CnH2n+1OH where n = 1, 2, 3…
Carboxylic acid
CnH2n+1COOH , n=0,1,2…
Ester
CmH2m+1COOCnH2n+1
Functional group Single covalent bond Carbon-carbon double covalent bond, C = C -OH, hydroxyl group
Carboxyl group Carboxylate group
Isomers are compounds with the same molecular formula but different structural formulae.
29.
OXIDATION
REDUCTION
+ oxygen
- oxygen
- hydrogen
+ hydrogen
- electron
+ electron
+ oxidation number
- Oxidation number
Reducing Agent
Oxidising Agent
30.
Heat of precipitation is the heat change when one mole of a precipitate is formed.
31.
Heat of displacement is the heat change when one mole of a metal is displaced from its salt solution by a more electropositive metal.
32.
Heat of neutralization is the heat change when one mole of water is formed from the reaction between an acid and an alkali.
33.
Heat of combustion is the heat change when one mole of a substance is completely burnt in oxygen under standard condition. All the heat of reaction, unit = KJ/mol
34.
Fuel value is the amount of heat energy given out when one gram of the fuel is completely burnt in excess of oxygen. Unit : kJ/gram
35.
FORMULA: 𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠 6.02 𝑥 1023
𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑚𝑎𝑠𝑠 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠
𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑣𝑜𝑙𝑢𝑚𝑒 𝑚𝑜𝑙𝑎𝑟 𝑣𝑜𝑙𝑢𝑚𝑒
Num. of moles = MV / 1000
The proton number of an atom is the number of protons in the nucleus of an atom.
2.
The nucleon number of an atom is the sum of the number of protons and neutrons in the atom.
3.
Isotopes are atoms of the same element with same proton number but different nucleon numbers.
4.
Molecular formula of a compound shows the actual number of atoms of each element that are present in a molecule of the compound.
5.
Empirical formula of a compound shows the simplest whole number ratio of atoms of each element present in the compound.
6.
Ionic bond is the chemical bond formed through the transfer of electrons from metal atoms to non-metal atoms to achieve the stable octet electron arrangement.
7.
Ionic compound consist of positive ions and negative ions which are held by strong electrostatic forces of attraction.
8.
Covalent bond is the chemical bond formed through the sharing of electrons between non metal atoms to achieve the stable duplet or octet electron arrangement.
9.
Covalent compound consists of neutral molecules which are held by weak intermolecular forces (Van der Waals).
10.
Electrolytes are substances that can conduct electricity when they are in molten states or aqueous solution and undergo chemical changes. Electrolytes are ionic compounds which contain freely moved ions and thus, they are able to conduct electricity.
11.
Electrolysis is a process whereby compounds in either molten or aqueous state are broken down into their constituent by passing electricity through them.
12.
An acid is a substance which ionises or dissociates in water to produce hydrogen ion, H+.
13.
A base is a substance which ionises or dissociates in water to produce hydroxide ion, OH-.
14.
An alkali is a base which is soluble in water and ionises or dissociates to produce hydroxide ion, OH-.
15.
Monoprotic acid is an acids which ionizes in water to produce 1 mol of H+ ion. Example: Hydrochloric acid – HCl, Nitric acid – HNO3
16.
Diprotic acid is an acid which ionizes in water to produce 2 mol of H+ ion. Example : Sulphuric acid – H2SO4
17.
Strong alkali is an alkali which ionises (dissociates) completely in water to form high concentration of hydroxide ions, OH-.
18.
Weak alkali is an alkali which ionises (dissociates) partially in water to form low concentration of hydroxide ions, OH-.
19.
Strong acid is an acid which ionises (dissociates) completely in water to form high concentration of hydrogen ions, H+.
20.
Weak acid is an acid which ionises (dissociates) partially in water to form low concentration of hydrogen ions, H+.
21.
An alloy is a mixture of two or more elements in a certain composition in which the major component is a metal.
22.
Polymers are a long chain molecule made by joining together lots of smaller repeating molecules called monomers through a process called polymerisation.
23.
Rate of reaction is the speed at which reactants are converted into the products in a chemical reaction OR the change in the quantity of reactants or products per unit time.
24.
Factors Affecting Rate of Reaction Total Surface Area Temperature Concentration Pressure Presence of Catalysts
25.
Catalyst is a substance that can change / speed up the rate of reaction but remains chemically unchanged at the end of the reaction.
26.
Activation Energy, Ea is the minimum energy the colliding particles must have before collision between them can result in chemical reaction.
27.
28.
Compounds Alkanes Alkenes
General formula CnH2n+2 CnH2n, where n = 2, 3 …
Alcohol
CnH2n+1OH where n = 1, 2, 3…
Carboxylic acid
CnH2n+1COOH , n=0,1,2…
Ester
CmH2m+1COOCnH2n+1
Functional group Single covalent bond Carbon-carbon double covalent bond, C = C -OH, hydroxyl group
Carboxyl group Carboxylate group
Isomers are compounds with the same molecular formula but different structural formulae.
29.
OXIDATION
REDUCTION
+ oxygen
- oxygen
- hydrogen
+ hydrogen
- electron
+ electron
+ oxidation number
- Oxidation number
Reducing Agent
Oxidising Agent
30.
Heat of precipitation is the heat change when one mole of a precipitate is formed.
31.
Heat of displacement is the heat change when one mole of a metal is displaced from its salt solution by a more electropositive metal.
32.
Heat of neutralization is the heat change when one mole of water is formed from the reaction between an acid and an alkali.
33.
Heat of combustion is the heat change when one mole of a substance is completely burnt in oxygen under standard condition. All the heat of reaction, unit = KJ/mol
34.
Fuel value is the amount of heat energy given out when one gram of the fuel is completely burnt in excess of oxygen. Unit : kJ/gram
35.
FORMULA: 𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠 6.02 𝑥 1023
𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑚𝑎𝑠𝑠 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠
𝑛𝑢𝑚. 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 =
𝑣𝑜𝑙𝑢𝑚𝑒 𝑚𝑜𝑙𝑎𝑟 𝑣𝑜𝑙𝑢𝑚𝑒
Num. of moles = MV / 1000
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