[🧪] Definitions Flashcards

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1
Q

Define:

first ionisation energy

A

The amount of energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of uni-positive ions.

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2
Q

Define:

isotope

A

An atom of the same element with the same number of protons but different number of neutrons.

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3
Q

Define:

unified atomic mass unit

A

One twelfth of the mass of a C₁₂ atom

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4
Q

Define:

relative atomic mass

A

the average mass of an atom of an element compared to one twelfth of the mass of a C₁₂ atom.

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5
Q

Define:

relative isotopic mass

A

The mass of an isotope of an element compared to one twelfth of the mass of a C₁₂ atom.

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6
Q

Define:

relative molecular mass

A

The sum of the relative atomic masses of each atom in a molecule.

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7
Q

Define:

relative formula mass

A

The sum of the relative atomic masses of each ion in the formula of an ionic compound compared to one twelfth of the mass of a C₁₂ atom.

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8
Q

Define:

mole

A

A mole of a substance is one Avogadro’s constant of particles in the substance.

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9
Q

Define

atomic orbitals

A

regions of space outside the nucleus that can be occupied by a maximum of two electrons

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10
Q

Define

covalent atomic radius

A

half the distance between two nuclei of covalently bonded atoms of the same type

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11
Q

Define

bond energy

A

the energy required to break one mole of a particular covalent bond in the gaseous state

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12
Q

Define:

bond length

A

the internuclear distance of two covalently bonded atoms

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13
Q

Define:

bond polarity

A

the partial separation of charge when two different atoms are joined by a covalent bond

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14
Q

Define:

covalent bond

A

The electrostatic forces of attraction between the nuclei of two atoms and a shared pair of electrons

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15
Q

Define:

ionic bond

A

The electrostatic forces of attraction between oppositely charged ions.

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16
Q

Define:

metallic bond

A

the electrostatic forces of attraction between positive metal ions and delocalised electrons

17
Q

Define:

electronegativity

A

the power of an atom to attract electrons towards itself

18
Q

Standard enthalpy change of reaction

A

the amount of heat energy released or absorbed when one mole of a substance is formed or reacted in a chemical reaction under standard conditions

19
Q

Standard enthalpy change of formation

A

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

20
Q

Standard enthalpy change of combustion

A

the amount of energy released when one mole of a substance is completely burned in excess oxygen under standard conditions

21
Q

Define

transition state

A

the stage in a reaction at which chemical bonds are partially broken and formed

22
Q

Define

average bond enthalpy

A

the energy needed to break one mole of bonds in a gaseous molecule averaged over similar compounds

23
Q

Define

disproportionation reaction

A

A disproportionation reaction is a type of redox reaction where a species is simultaneously oxidised and reduced