Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry unit 1 > Chemistry Unit 1 Definitions > Flashcards

Chemistry Unit 1 Definitions Flashcards

0
Q

Precipitation Reaction

A

The formation of a solid from a solution during a chemical reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

Halogens

A

Group VII elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Oxidising Agent

A

A reagent that oxidised another species.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Halides

A

Negative ions of group VII elements.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Electronegativity

A

The ability of an atom to attract a bonded pair of electrons in a covalent bond towards itself.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Disproportionation Reaction

A

The oxidation and reduction of the same element in a redox reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Reducing Agent

A

A reagent that reduces another species.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Displacement Reaction

A

A reaction in which a more reactive element displaces a less reactive element from an aqueous solution in the latter’s ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Reducing Agent

A

A species that causes reduction in another species, whilst itself is being oxidised.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Oxidising Agent

A

A species that causes oxidation in another species, whilst itself is being reduced.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Reduction

A

Gain of electrons or a decrease in oxidation number.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Thermal Decomposition

A

The breaking up of a chemical substance with heat into at least two chemical substances.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Oxidation Number or Oxidation State

A

A measure of the number of electrons that an atom uses to bond with atoms of another element.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Redox Reaction

A

A reaction where both oxidation and reduction takes place.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Oxidation

A

Loss of electrons or an increase in oxidation numbers.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

First Ionisation Energy

A

The minimum amount of energy required to remove one electron from each atom in one one mole of gaseous atoms to form 1+ ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Second Ionisation Energy

A

The minimum amount of energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form 2+ ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Periodicity

A

Repeating patterns of properties across a period.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Electronegativity

A

The ability of an atom to attract a bonded pair of electrons in a covalent bond towards itself.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Alkali

A

A type of base that dissolves in water forming hydroxide (OH-)(aq) ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Hydrated

A

The compound in question contains water.

21
Q

Salt

A

A chemical compound formed from an acid, when a H+ ion from the acid has been replaced by a metal ion or another positive ion, such as ammonium ion NH4+.

22
Q

Base

A

A species that is a proton ( H+) acceptor.

23
Q

Anhydrous

A

The compound on question contains no water.

24
Q

Water Of Crystallisation

A

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

25
Q

Acid

A

A species that is a proton ( H + ) donor.

26
Q

Hydrogen Bonding

A

A strong dipole- dipole attraction between an electron-deficient hydrogen atom on one molecule and a lone pair of electrons

27
Q

Dipole- Dipole Interactions (permanent dipole)

A

An attractive force between permanent dipoles in neighbouring polar molecules.

28
Q

Metallic Bond

A

The electrostatic attraction between positive meta ions and delocalised electrons.

29
Q

Ionic Bond

A

The electrostatic attraction between oppositely charged ions.

30
Q

Coordinate Bond

A

A shared pair of electrons which has been provided by one of the bonding atoms only.

31
Q

Van Der Waals Forces

A

Very weak attractive forces between induced dipoles in neighbouring molecules.w

32
Q

Electronegativity

A

A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond.

33
Q

Covalent Bond

A

A bond formed by a shared paired of electrons.

34
Q

Molecular Formula

A

The number of atoms of each element in a molecule.

35
Q

Molar Mass

A

The mass per mole of a substance.

36
Q

Amount Of Substance

A

The quantity whose unit is the mole

37
Q

Mole

A

The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope.

38
Q

Avagadro’s Constant

A

The number of atoms per mole of the carbon 12 isotope.

39
Q

Empirical Formula

A

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

40
Q

Relative Isotopic Mass

A

The mass of an atom of an isotope compared to 1/12th the average mass of an atom of carbon-12.

41
Q

Relative Atomic Mass

A

The average mass of an atom of an element compared to 1/12th the average mass of an element of carbon-12.

42
Q

Second Ionisation Energy

A

The minimum amount of energy required to remove one electron from each ion in one mole of gaseous atoms to form 2+ ions.

43
Q

First Ionisation Energy

A

The minimum amount of energy required to remove one electron from each atom in one mole of gaseous atoms to produce 1+ ion.

44
Q

Atomic Number

A

The number of protons in the nucleus.

45
Q

Isotope

A

Atoms of an element with different number of neutrons.

46
Q

Relative Formula Mass

A

The average mass of a formula of a compound compared to 1/12th the average mass of an atom of carbon-12.

47
Q

Relative Molecular Mass

A

The average mass of a molecule compared to 1/12th the mass of an atom of carbon-12.

48
Q

Atomic Orbital

A

The region within an atom that can hold up to 2 electrons with opposite spins.

49
Q

Mass Number

A

The number of protons and neutrons in the nucleus.

Chemistry unit 1 (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions