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Chemistry > Bonding 3 > Flashcards

Bonding 3 Flashcards

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1
Q

Positive and negative ions are formed

A

Ionic

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2
Q

Ionic lattice

A

Electrostatic forces between oppositely charged ions.

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3
Q

Two non-metals

A

Covalent

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4
Q

Share their electrons

A

Covalent

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5
Q

Dative covalent bonding

A

Atom that accepts the electron pair is an atom that doesn’t have a filled outer main shell ( electron-deficient)
Atom that is donating the electron has a pair of electrons (lone pair)

(contains a shared pair of electrons with both electrons supplied by one atom)

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6
Q

Delocalised electrons

A

Metallic bonding

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7
Q

Good conductors of heat and electricity

A
  • sea of delocalised electron

- high thermal conductivities

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8
Q

Strength of metals

A
  • charge of ions

- size of ion

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9
Q

Malleable and ductile

A

Layers can slide over each other

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10
Q

High melting point

A

Giant structure

Strong attraction between metal ions and sea of delocalised electrons

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11
Q

Electronegativity

A

The power of an atom to attract the electron density in a covalent bond towards itself

(Electronegativity as the power of an atom to attract the pair of electrons in a covalent bond)

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12
Q

What element is the most electronegative?

A

Fluorine

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13
Q

Metal and non-metal

A

Ionic

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14
Q

Polar

A

Greater the difference in electronegativity the more polar the bond is

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15
Q

Metallic bonding

A

(Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice)
Positive metal ion and an electron
Sea of delocalised electrons
Ions ( and electrons) repel each other

Good conductor of heat and electricity

Strength
Increase charge of the ion

Malleable and ductile ( layers slide over each other)

High melting point

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16
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions ( creates a ion lattice )
Giant structures - high melting point
Conduct electricity
Brittle and shatter ( small displacement causes two positive ions ( or electrons) to touch each other and repel each other

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17
Q

Covalent bonding

A

Pair of electrons are shared
Strong covalent bonds are only between the atoms with in the molecule
Weak attraction between molecules so not much energy is needed

Poor conductor

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18
Q

Co-ordinate bonding

A

Covalent bonding in which both the electrons in the bond come from one of the atoms in the bond

One of the atoms would have a lone pair

Represented by an arrow

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19
Q

Electronegatively increases across a period

A

Increased nuclear charge
Amount of shielding stays the same
Atoms are smaller because the positive charge makes in smaller

20
Q

Electronegatively decrease down a group

A

More distance from the nucleus
Amount of shielding increases
Nuclear charge increases but is counteracted by the shielding effect and distance

21
Q

Van der waals

A

At any time the electrons can be anywhere. At any moment it could have a dipole at any time

Closer together the molecules the stronger the force
Larger molecules have larger electron clouds meaning stronger van der waal force

22
Q

Dipole-dipole

A

Permeant dipole ( one is positives and one is negative)

Opposite charges attract and repel each other

23
Q

Hydrogen bonding

A

Fluorine
Oxygen
Nitrogen

Very electronegative

24
Q

Importance of hydrogen bonding

A

Molecules are slightly less closely packed than a liquid so it is less dense than water
Forms on top of ponds
Insulates ponds

25
Q

Ironing

A

Ironing provides heat to break hydrogen bonds in the crumpled material and pressure to force the molecules into a new postion

26
Q

DNA

A

Stores and copies genetic information that makes offspring like the parents (double-stranded helix) —- two stands are held together by hydrogen bonding

When the cells divid (replicate) the hydrogen bond break. You get a copy of the original helix

27
Q

Enthalpy change

A

A measure of heat energy given out or taken in when a chemical or physical change would occur at constant pressure

28
Q

Enthalpy change of melting

A

Amount of energy needed to weaken the forces that act between the particles

Per moles

29
Q

Enthalpy change of vaporisation

A

Amount of energy to break all the intermolecular bonds between molecular

Per mole

30
Q

Ionic crystals

A

NaCl
Strong electrostatic attraction between oppositely charged ions

Melting point 801 c

31
Q

Metallic crystals

A

Mg

Lattice has a high melting point

32
Q

Molecular crystals

Iodine

A

Held in regular array by intermolecular forces

114 C
Large number of electrons

(Soft/easy to break , low melting point, doesn’t conduct electricity)

33
Q

Macromolecular crystals

A

Covalent bonds
String bonds
High melting point

34
Q

Diamond

A

Bonds spread through the structure 4 carbon bonds (bond angle = 109.5)
Very hard material
High melting point 3700k+
No electrical charge

35
Q

Graphite

A

3 Strong covalent bonds
Weak van der waal forces between 1 pair of electrons ( bond angle = 120)
Two dimensional layer of linked hexagon of carbon atoms
(Spare ) electron in the p-orbital -delocalised electron
High melting temperature
Conducts electricity

36
Q

Electronegatively depends on

A

Nuclear charge
Distance between the nucleus and outer shell electrons
Shielding

37
Q

sulfate

A

SO4

charge of -2

38
Q

hydroxide

A

OH-

39
Q

nitrate

A

NO3-

40
Q

carbonate

A

CO3 -2

41
Q

ammonium

A

NH4+

42
Q

drawing bonds

A

covalent bond using a line

co-ordinate bond using an arrow

43
Q

ice

A

Ice is a good example of a hydrogen bonded solid.

44
Q

2 pair of lone electrons

A

Lone pair–lone pair repulsion is greater than lone pair–bond pair repulsion, which is greater than bond pair–bond pair repulsion

45
Q

how do electrons arrange themselves?

A

Pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repulsion

46
Q

how polar bonds form

A

The electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical. This produces a polar covalent bond, and may cause a molecule to have a permanent dipole

Chemistry (20 decks)

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