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Chemistry Module 2 > Definitions > Flashcards

Definitions Flashcards

(77 cards)

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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
tmoms anhydrous
Crystalline compound containing no waters of crystallization
26
Atom economy
Measure of the amount of starting materials that end up as useful products High atom economy means more sustainable as less waste produced
27
Avogadro constant
Number of particles per mole of substance
28
Composition by mass
Relative mass of each element in a compound
29
Empirical formula
Simplistic whole number ratio of atoms of each element present in a compound
30
Hydrated
Crystalline compound that contains water
31
Ideal gas
Gas that has molecules that occupy negligible space with no interactions between them
32
Molar gas volume
Volume of 1 mole of gas
33
Mole
Amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon-12
34
Molecular formula
Number and type of atoms of each element in a molecule
35
Percentage yield
Percentage ratio of the actual yield compared with the theoretical yield
36
Stoichiometry
Relative quantities of substances in a reaction
37
Water of crystallization
Water molecules that form part of the crystalline structure of a compound
38
Acid
Compounds that release H+ ions in aqueous solution
39
Alkali
Water soluble bases, release OH- ions into aqueous solution
40
Base
Substance that can accept H+ ions from another substance
41
Neutralization
Reaction between H+ andOH- forming water
42
Strong acid
Acid that completely dissociates in solution
43
Titration
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
Weak acid
Acid that only partially dissociates in solution
45
Oxidation
Loss of electrons/ increase in oxidation number
46
Oxidation number
Number that represents the number of electrons lost of gained by an atom of an element Positive is a loss
47
Redox reaction q
Reaction in which one element is oxidizes and another is reduced
48
Reduction
Gain of electrons/ decrease in oxidation number
49
Atomic orbital
Region of high probability in which 2 electron with opposite spin can occupy
50
Electronic configuration
Arrangement of electrons into orbitals and energy levels around the nucleus of an atom/ion
51
Energy level
Shell electron is in
52
Shell
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
Sub-shell
Sub division of the electronic shells into different orbitals S,p,d and f
54
Average one enthalpy
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
Bonding pair
Pair of outer shell electrons involved in bonding
56
Covalent bond
Strong bond formed between 2 atoms due to the electrostatic attraction between a shared pair of electrons and the atomic nuclei
57
Dative covalent (coordinate bond)
Type of covalent bond in which both of the electrons in the shared pair come from 1 atom
58
Electronegativity
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
Electron pair repulsion theory
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
Hydrogen bonding
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
d intermolecular forces
Interactions between differerent molecules | Include permanent dipole dipole, induced dipole dipole and hydrogen bonding
62
Ionic bond
Electrostatic attraction between positive and negative charged ions
63
Ionic lattice
Giant structure in which oppositely charged ios are strongly attracted in all directions
64
Linear
Shape of the molecule in which the central atom has 2 bonding pairs
65
London forces
Induced dipole dipole Random movement of electrons creates a temporary dipole in one molecule which then induces a dipole in a neighboring molecule
66
Lone pair
Pair of outer shell electrons not involved in bonding
67
Macroscopic properties
Properties of a bulk material rather than individual atoms/molecules that make up the material
68
Non-linear
Shape of the molecule in which the central atom has 2 bonding pairs and 2 one pairs
69
Octahedral
Shape of the molecule in whic hthe central atom has 6 bonding pairs
70
Permanent dipole
Permanent uneve distribution of charge
71
Polar bond
Covalent bond that has a permanent dipole due to the different electronegativities of the atoms that make up the bond
72
Polar molecule
Contains polar bonds with dipoles that don’t cancel out due to their direction Unsymmetrica
73
l pyramidal
Shape of the molecule in which the central atom has 3 bonding pairs and 1 lone pair
74
Simple molecular lattice
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
Tetrahedral
Shape of a molecule in which the central atom has 4 bonding pairs
76
Trigonal bipyramidal
Shape of a molecule in why the central atom has 5 bonding pairs
77
Trigonal planar
Shape of a molecule in which the central atoms has 3 bonding pairs

Chemistry Module 2 (8 decks)

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