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Chemistry Module 2 > Definitions > Flashcards

Definitions Flashcards

1
Q

Atomic number

A

Number of protons in the nucleus of an atom

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2
Q

Bohr model

A

Describes an atom as a small dense nucleus with electrons orbiting around th nucleus
Explains the difference periodic properties of atoms

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3
Q

Electron

A

Negatively charged subatomic particle which orbits the nucleus at various energy levels
Relative mass is 1/1836

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4
Q

Ion

A

Charged atom or molecule

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5
Q

Isotope

A

Atoms of the same element with the same number of protons and electrons and different numbers of neutrons
Have different masses

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6
Q

Mass number

A

Total number of protons and neutrons in the nucleus of an atom

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7
Q

Mass spectrometry

A

Instrument which gives accurate information about relative isotopic mass and the relatie abundance of isotopes

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8
Q

Neutro

A

Neutral subatomic particle found in the nucleus of an atom

Relative mas is 1

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9
Q

Proton

A

Positively charged subatomic particle found in the nucleus of an atom
Relative mass is 1

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10
Q

Relative abundance

A

Amount of one substance compared to another

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11
Q

Relative atomic mass

A

Weighted mean mass of an atom compared to 1/12th mass of an atom of carbon-12

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12
Q

Relative isotopic mass

A

Mass of an atom of an isotope compared to 1/12th mass of an atom of carbon-12

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13
Q

Relative formula mass

A

Mass of the formula unit of a compound with a giant structure

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14
Q

Relativel molcular mass

A

Mass of a simple molecule

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15
Q

Ammonium ion

A

NH4 +

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16
Q

Carbonate ion

A

CO3 2-

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17
Q

Hydroxide ion

A

OH-

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18
Q

Ionic compound

A

Compound which is made up of oppositively charged ions that are held together by electrostatic forces of attraction

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19
Q

Nitrate ion

A

NO3 -

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20
Q

Silver ion

A

Ag +

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21
Q

State symbols

A

Symbols within a chemical equation which indicate the state of each compound under the reaction conditions

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22
Q

Sulfate ion

A

SO4 2-

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23
Q

Zinc ion

A

Zn 2+

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24
Q

Amount of substance

A

Quantity that has moles as its units

Used as a way of counting a

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25
Q

tmoms anhydrous

A

Crystalline compound containing no waters of crystallization

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26
Q

Atom economy

A

Measure of the amount of starting materials that end up as useful products
High atom economy means more sustainable as less waste produced

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27
Q

Avogadro constant

A

Number of particles per mole of substance

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28
Q

Composition by mass

A

Relative mass of each element in a compound

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29
Q

Empirical formula

A

Simplistic whole number ratio of atoms of each element present in a compound

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30
Q

Hydrated

A

Crystalline compound that contains water

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31
Q

Ideal gas

A

Gas that has molecules that occupy negligible space with no interactions between them

32
Q

Molar gas volume

A

Volume of 1 mole of gas

33
Q

Mole

A

Amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon-12

34
Q

Molecular formula

A

Number and type of atoms of each element in a molecule

35
Q

Percentage yield

A

Percentage ratio of the actual yield compared with the theoretical yield

36
Q

Stoichiometry

A

Relative quantities of substances in a reaction

37
Q

Water of crystallization

A

Water molecules that form part of the crystalline structure of a compound

38
Q

Acid

A

Compounds that release H+ ions in aqueous solution

39
Q

Alkali

A

Water soluble bases, release OH- ions into aqueous solution

40
Q

Base

A

Substance that can accept H+ ions from another substance

41
Q

Neutralization

A

Reaction between H+ andOH- forming water

42
Q

Strong acid

A

Acid that completely dissociates in solution

43
Q

Titration

A

Technique used to determine the amount of one solution of a known conc required to completely react with a known volume of another solution of unknown concentration

44
Q

Weak acid

A

Acid that only partially dissociates in solution

45
Q

Oxidation

A

Loss of electrons/ increase in oxidation number

46
Q

Oxidation number

A

Number that represents the number of electrons lost of gained by an atom of an element
Positive is a loss

47
Q

Redox reaction q

A

Reaction in which one element is oxidizes and another is reduced

48
Q

Reduction

A

Gain of electrons/ decrease in oxidation number

49
Q

Atomic orbital

A

Region of high probability in which 2 electron with opposite spin can occupy

50
Q

Electronic configuration

A

Arrangement of electrons into orbitals and energy levels around the nucleus of an atom/ion

51
Q

Energy level

A

Shell electron is in

52
Q

Shell

A

Orbit that an orbital is in around the nucleus of an atom, shell closest to nucleus is the first shell, outermost is the valence shell

53
Q

Sub-shell

A

Sub division of the electronic shells into different orbitals
S,p,d and f

54
Q

Average one enthalpy

A

Average energy required to break a bond, used as a measurement of the strength of a covalent bond, measured using a variety of molecules that contain a specific bond

55
Q

Bonding pair

A

Pair of outer shell electrons involved in bonding

56
Q

Covalent bond

A

Strong bond formed between 2 atoms due to the electrostatic attraction between a shared pair of electrons and the atomic nuclei

57
Q

Dative covalent (coordinate bond)

A

Type of covalent bond in which both of the electrons in the shared pair come from 1 atom

58
Q

Electronegativity

A

Tendency of an atom to tract bonding electrons in a covalent bond, often quantified using Paulina’s electrognegativity values, electronegativity increases towards F in the periodic table

59
Q

Electron pair repulsion theory

A

Pair of electrons around a nucleus repel each other so the shape that a molecule adopts has these pairs of electrons positioned as far apart as possible, lone pairs offer more repulsion than bonding pairs as they are closer to the nucleus of the central atom

60
Q

Hydrogen bonding

A

Type of intermolecular bonding that occurs between molecules containing n,o, f and H atom of the previous elements
Lone pair on the electronegative atom allows the formation of a hydrogen bon

61
Q

d intermolecular forces

A

Interactions between differerent molecules

Include permanent dipole dipole, induced dipole dipole and hydrogen bonding

62
Q

Ionic bond

A

Electrostatic attraction between positive and negative charged ions

63
Q

Ionic lattice

A

Giant structure in which oppositely charged ios are strongly attracted in all directions

64
Q

Linear

A

Shape of the molecule in which the central atom has 2 bonding pairs

65
Q

London forces

A

Induced dipole dipole
Random movement of electrons creates a temporary dipole in one molecule which then induces a dipole in a neighboring molecule

66
Q

Lone pair

A

Pair of outer shell electrons not involved in bonding

67
Q

Macroscopic properties

A

Properties of a bulk material rather than individual atoms/molecules that make up the material

68
Q

Non-linear

A

Shape of the molecule in which the central atom has 2 bonding pairs and 2 one pairs

69
Q

Octahedral

A

Shape of the molecule in whic hthe central atom has 6 bonding pairs

70
Q

Permanent dipole

A

Permanent uneve distribution of charge

71
Q

Polar bond

A

Covalent bond that has a permanent dipole due to the different electronegativities of the atoms that make up the bond

72
Q

Polar molecule

A

Contains polar bonds with dipoles that don’t cancel out due to their direction
Unsymmetrica

73
Q

l pyramidal

A

Shape of the molecule in which the central atom has 3 bonding pairs and 1 lone pair

74
Q

Simple molecular lattice

A

Solid structure made up of covalently bonded molecules attracted by intermolecular force, relatively low melting and boiling points typically insoluble in water but soluble in organic solvents, don’t conduct electricity

75
Q

Tetrahedral

A

Shape of a molecule in which the central atom has 4 bonding pairs

76
Q

Trigonal bipyramidal

A

Shape of a molecule in why the central atom has 5 bonding pairs

77
Q

Trigonal planar

A

Shape of a molecule in which the central atoms has 3 bonding pairs

Chemistry Module 2 (8 decks)

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