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Chemistry > Bonding Ect. > Flashcards

Bonding Ect. Flashcards

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0
Q

ZONC 2/4 + angle

A

Bent (v shaped) 109

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1
Q

Group 7 Elements

A

Halogens

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2
Q

Metallic Bonding

A

The strong electrostatic force of attraction between positive ions and delocalised electrons that make up a metal

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3
Q

Melting point pp rule

A

The stronger the bond strength between particles, the more heat energy required to break it, thus the higher melting point

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5
Q

Electrostatic attraction

A

The attraction between positively charged and negatively charged particles

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6
Q

Polarity pp rule

A

Polar substances dissolve in polar solvents where non polar substances dissolve in non polar solvents

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7
Q

Group 8 Elements

A

Inert gases , Nobel gases

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7
Q

Isotope

A

Atoms of the same element but with different mass numbers

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8
Q

Electricity’s charged particles

A

Free moving delocalised electrons (as in metals) , mobile ions (as in molten or dissolved ionic substances)

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9
Q

Diamond

A

Carbon atoms , covalent

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10
Q

Solid structures

A

Lattice (network) , Molecular

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11
Q

Intramolecular Forces

A

The forces within the molecules are the covalent bonds linking atoms in individual molecules. These forces are very strong

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12
Q

Covalent Networks

A

Where all atoms in a three dimensional network are held together by strong covalent bonds.

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13
Q

ZONC 4/4 + angle

A

Tetrahedral 109

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14
Q

Bond strength

A

The stronger the bond between particles, the more heat required to break it - thus the higher it’s melting point

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15
Q

Ionic Solids

A

Ions attract each other electrostatically, so that each is surrounded by a group of oppositely charged ions forming a stable three dimensional lattice

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15
Q

Molecular Solids (discrete molecular substances)

A

Solids made of separate molecules packed together. There are two forces present - intramolecular and intermolecular

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17
Q

Bond Strength

A

The stronger the bond, the higher it’s melting point and boiling point

18
Q

Metallic Solids

A

Metals consist of a three dimensional array of metal atoms and delocalised electrons moving freely through the lattice.

19
Q

Non-Polar Covalent Bond

A

Formed by equal (or nearly equal) sharing of electrons between two non metal or metalloid atoms

20
Q

ZONC 3/3 + angle

A

Triangular planar 120

21
Q

Polar Covalent Bond

A

Formed by the uneven sharing of electrons between two non metals or metalloids

22
Q

ZONC 3/4 + angle

A

Trigonal pyramid 109

23
Q

Allotrope

A

Different physical form of element

24
Q

Particle Charge

A

A substance is able to conduct electricity if charged particles are free to move

25
Q

Ionic Bond

A

Formed by the transfer of electrons from a metal to a non metal

26
Q

Particles (6)

A

Protons , neutrons , electrons , atoms , molecules , ions

27
Q

Electron Shells

A

Energy levels

28
Q

Rule of distribution of electrons

A

Octet rule

29
Q

Intermolecular Forces

A

The forces between the molecules link individual molecules to each other. These forces are very week and determine the physical properties of discrete molecular substances.

30
Q

Hydrated ions

A

Separated ions surrounded by water molecules

Written as (aq) after symbol

32
Q

Conductivity pp rule

A

A substance is able to conduct electricity charged particles are free to move

34
Q

Conductivity

A

A substance can conduct electricity if charged particles are free to move

35
Q

ZONC 2/2 + angle

A

Linear 180

36
Q

ZONC 2/3 + angle

A

Bent (v shaped) 120

37
Q

Repulsion statement

A

These zones repel to give maximum separation

38
Q

Electronegativity difference

A

The difference in the pull of bonded atoms on the electrons they share

39
Q

Electronegative scale

A 
F or
O ur
Cl ass
N asty
Br ehaut
C an't
H elp
40
Q

Dipole

A

Charge separation that occurs across the polar bond

41
Q

Solubility in ionic substances

A

The strong ionic bonds holding ions together are overcome by attraction between the ions and the polar water molecules.
The ions separate.
The separated ions are surrounded by water molecules to form hydrated ions.

42
Q

Ionic solubility pp rule

A

The amount of lattice energy required to break up an ionic lattice so that hydrated ions can be produced, varies for different ionic compounds.

43
Q

Ionic solubility rule pt 2 (insoluble)

A

Ionic compounds are insoluble if more energy is required to separate the ions, than can be gained by forming hydrated ions.

44
Q

Ionic solubility rule pt 2 (soluble)

A

Ionic compounds are soluble if there is sufficient energy to separate the ions in the ionic lattice to form hydrated ions.

Chemistry (3 decks)

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