Key Words Flashcards

(35 cards)

0
Q

Molecular Formula

A

Actual number of atoms of each element in a molecule.

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1
Q

Empirical Formula

A

The simplest whole number ratio of atoms of each element present in a compound.

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2
Q

Heterolytic Fission

A

Breaking of a covalent bond, where both electrons go to one atom

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3
Q

Homologous Series

A

A series of organic compounds having the same function group but with each successive member differing by CH2

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4
Q

Structural Isomers

A

Compounds with the same molecular formula but different structural formula.

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5
Q

Stereoisomers

A

Compounds with the same structural formula but with a different arrangement of atoms in a space.

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6
Q

E/Z Isomerism

A

Restricted rotation about a double bond C=C.

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7
Q

Homolytic Fission

A

Breaking of a covalent bond where 1 electron goes to each atom.

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8
Q

Hydrocarbon

A

Compound containing only hydrogen and carbon.

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9
Q

Enthalpy Change of Reaction

A

The enthalpy change that occurs in a reaction in the molar quantities in a chemical equation under standard conditions in standard states.

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10
Q

Radical

A

Species with an unpaired electron.

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11
Q

Activation Energy

A

Minimum energy required in order to start a reaction by breaking bonds.

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12
Q

Enthalpy Change of Formation

A

The enthalpy change when a mole of compound is formed from its constituent elements in their standard states under standard conditions.

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13
Q

Le Chatelier’s Principle

A

When a system is in dynamic equilibrium and is subject to a change, the position will shift to minimise change.

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14
Q

Enthalpy Change of Combustion

A

The enthalpy change when one mole of substance is completely oxidised in an excess of oxygen under standard conditions and states.

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15
Q

Catalyst

A

Speeds up a reaction without being consumed by the overall reaction.

16
Q

Relative Atomic Mass

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon 12.

17
Q

Relative Isotopic Mass

A

The weighted mean mass of an atom of an isotope relative to 1/12th of the mass of an atom of carbon 12.

18
Q

Relative Molecular Mass

A

The mass of one molecule relative to 1/12th of he mass of an atom of carbon 12.

19
Q

Relative Formula Mass

A

Weighted mean mass of a formula unit relative to 1/12th of a mass of an atom of carbon 12.

20
Q

Isotopes

A

Different neutron number. Same number of protons and electrons.

21
Q

Hydrated

A

Crystalline structure that contains water molecules.

22
Q

Anhydrous

A

Without water.

23
Q

Water of Crystallisation

A

Water molecules that form an essential part of the crystalline structure of a compound.

24
Orbital
A region within an atom that can hold up to two electrons with opposite spins.
25
Covalent Bond
A bond formed by a shared pair of electrons.
26
Dative Bonding
Both electrons come from same atom.
27
Lone Pair
An outer shell pair of electrons that aren't involved in bonding.
28
Electronegativity
Measure of the ability of an atom to attract electrons in a covalent bond.
29
Ionic Bond
The electrostatic attraction between oppositely charged ions.
30
Metallic Bond
The electrostatic attraction between positive ions and negative electrons.
31
First Ionisation Energy
The energy needed to remove an electron from each atom in one mole of gaseous atoms.
32
Periodicity
Repeating patterns across the periodic table
33
One Mole of Substance
The amount of substance which contains as many particles as there are carbon atoms in 12g of Carbon 12
34
Successive Ionisation Energy
The energy needed to remove each subsequent electron from each ion in 1 mole of positively charged gaseous ions.