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Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

Energy levels

A

Regions of space where electrons have fixed energies

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2
Q

Ground state

A

When all electrons in an atom are in there lowest energy state

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3
Q

Orbital

A

An orbital is a three dimensional region around the nucleus where there is a high probability of finding an electron with a certain amount of energy

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4
Q

Isotopes

A

Isotopes are different atoms of the same element with the same atomic number but different mass numbers

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5
Q

Relative atomic mass (Ar)

A

The relative atomic mass (Ar) is a number that compares the average mass of an atom with the mass of the C-12 atom taken to be 12 units

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6
Q

Cation

A

A positive ion and forms when an atom loses an electron

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7
Q

Anion

A

Is a negative ion and forms when an atom gains an electron

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8
Q

Ionization energy

A

The ionization energy is the minimum amount of energy required to remove an electron from an atom in the gas phase

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9
Q

Chemical bonding

A

Chemical bonding is the process by which atoms bond with each other and in this way achieve a noble gas configuration, with low potential energy

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10
Q

A molecule

A

A molecule is a group of two or more atoms which are bonded together strongly enough to behave as a single unit in a chemical reaction

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11
Q

Bond strength

A

Bond strength is the amount of energy needed to break a chemical bond

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12
Q

Valency

A

Valency is a measure of the number of chemical bonds formed by the atoms of a given element

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13
Q

Covalent bond

A

A covalent bond is a sharing of electrons between two non-metal atoms, forming a molecule

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14
Q

Electronegativity

A

Electronegativity is an indication of the attraction that an atom exerts on a shared electron pair

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15
Q

Non-polar covalent bond

A

A non-polar covalent bond (pure covalent bond) is a covalent bond where there is an equal sharing of electrons

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16
Q

Polar covalent bond

A

A polar covalent bond is a covalent bond where there is an unequal sharing of electrons leading to a dipole forming (as a result of electronegativity difference)

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17
Q

Intermolecular force

A

An intermolecular force is a weak force of attraction between molecules or between atoms of a noble gas

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18
Q

Van der waals forces

A

The attractive forces between molecules are collectively called Van der Waals forces

19
Q

Dipole-dipole

A

Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

20
Q

Dipole-induced dipole

A

A dipole-induced dipole attraction is a weak attraction that results when a polar molecule induces a dipole in an atom or in a non-polar molecule by disturbing the arrangement of electrons in the non-polar species

21
Q

London forces

A

The London force is the weakest intermolecular force. It is a temporary attractive force that results when the electrons in two adjacent atoms or molecules occupy positions that make the atoms or molecules form temporary dipoles. London forces exist between two non-polar molecules or between atoms of noble gasses.

22
Q

Hydrogen bonding

A

Hydrogen bonding results from the attractive force between a hydrogen atom covalently bonded to a small, very electronegative atom such as an N, O or F atom

23
Q

Ionic bond

A

An ionic bond forms due to a transfer of electrons and subsequent electrostatic attraction

24
Q

Crystal lattice

A

A crystal lattice is a regular 3D structure of particles

25
Q

Ion-dipole

A

An ion-dipole is an attractive force that results from the electrostatic attraction between an ion and a dipole

26
Q

Ion-induced dipole

A

And ion-induced dipole attraction is a weak attraction that results when the approach of an ion induces a dipole in an atom or NP molecule by disturbing the arrangement of electrons in the NP species

27
Q

Metallic bond

A

A metallic bond is between a positive kernel and a sea of delocalised electrons

28
Q

Allotropes

A

Allotropes are different forms of the same element

29
Q

Dative covalent bond

A

A dative covalent bond (also called a coordinate bond) is a a covalent bond in which both electrons come from the same atom

30
Q

Heterogenous mixture

A

In a heterogeneous mixture the substances are in different phases eg. Sand and water

31
Q

Homogeneous mixture

A

In a Homogeneous mixture only one phase can be distinguished eg. Salt in water

32
Q

Solution

A

A solution is a homogeneous mixture of two or more pure substances of which the composition can be varied

33
Q

The mole

A

The mole (n) is the number of elementary particles that is equal to the number of carbon atoms in 12g of carbon-12

34
Q

Avogadros constant

A

(Na) 1 mole of carbon-12 is 6,02 x 10’23

35
Q

The molar mass (M)

A

The molar mass (M) of a compound is the mass of one mole of that compound. The unit of molar mass is g•Mol -1

36
Q

Percentage composition

A

The percentage composition of a compound is the relative measure of the mass of each different element present in the compound

37
Q

Dissociation

A

Dissociation is when ionic substances dissolve in water

38
Q

Ionization

A

When certain polar covalent molecules dissolve in water they form ions

39
Q

Standard temperature

A

0•C / 273K

40
Q

Standard pressure

A

1,013 x 10’5 Pa

41
Q

Volume of 1 mole of any gas at STP

A

22,4 dm’3. Known as molar gas volume at STP (Vm)

42
Q

Temperature of gas

A

The temperature of a gas is directly proportional to the average kinetic energy of the particles of the gas

43
Q

Dipole

A

The separation of charge between two covalently bonded atoms

Chemistry (4 decks)

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