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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is ionic bonding , give an example

A

Attraction between oppositely charged ions formed by the transfer of electrons from one atom to the other eg NaCl

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2
Q

What is covalent bonding , give an example

A

Pair of e- shared between two atoms eg H20

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3
Q

Definition of dative covalent bond and how you would represent one?

A

Pair of e- shared between two atoms one of which provides both electrons to the bond, arrow from atom with lone pair and atom with no electrons

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4
Q

What is metallic bonding

A

Attraction between cations and a sea of electrons

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5
Q

Why does a dative covalent bond occur

A

Covalent bonding happens because the electrons are more stable when attracted to two nuclei than when attracted to only one.

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6
Q

Why does metallic bonding occur

A

Metallic bonding happens because the electrons are attracted to more than one nucleus and hence more stable. The electrons are said to be delocalized – they are not attached to a atom=free

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7
Q

What happens to electronegativity across a period

A

Electronegativity increases across a period as the nuclear charge on the atoms increases but the shielding stays the same,

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8
Q

What happens to electronegativity down a group

A

Electronegativity decreases down a group as the number of shells increases, so shielding increases and the electrons are less strongly attracted to the atom.

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9
Q

Why are noble gases not electronegative

A

They do not form bonds

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10
Q

What charges are in Polar covalent bond?

A

Delta + and -

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11
Q

How are all bonds assumed covalent

A

Power of electro negativity from one atom in comparison too the other shows you which type- eg ionic one atom is more more electronegative hence is presented as gaining an electron

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12
Q

Solid structure..

A

Tightly packed , ordered infinitely repeating lattice

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13
Q

What kind of structure does ionic bonding make

A

lattice is an infinite and repeating arrangement of particles. All the anions are surrounded by cations and all the cations are surrounded by anions.

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14
Q

How can you increase melting and boiling point in ionic compounds

A

Higher charge
Smaller ions

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15
Q

Can ionic compounds conduct electricity

A

In solid =no act as good insulators
Liquid=yes ions can move

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16
Q

Why are ionic compounds strong

A

Ions cannot slip or move over each other

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17
Q

Metallic bonding forms a lattice but can conduct electricity, why?

A

Delocalised e- carry charge

18
Q

How to increase mp and bp of metallic compounds

A

Smaller ions with higher charge

19
Q

Why are metals soft,malleable and ductile

A

n-directional, it does not really matter how the cations are oriented relative to each other. The metal cations can be moved around and there will still be delocalized electrons available to hold the cations together. The metal cations can thus slip over each other fairly easily.

20
Q

What is a sigma bond?

A

σ-bond is a bond resulting from direct overlap of two orbitals along the internuclear axis.
All single bonds between two atoms are σ-bonds.

21
Q

Why can you only have one sigma bond between 2 atoms

A

another would force too many electrons into a small space and generate repulsion.

22
Q

What is a pi bond?

A

If two orbitals overlap above and below (or behind and in front of) the internuclear axis, then a π-bond is formed.
+ or
A π-bond is a bond resulting from overlap of atomic orbitals above and below the internuclear axis.
All double bonds consist of a σ-bond and a π-bond.

23
Q

Example of molecular substances

A

CH4,Cl2,NH3

24
Q

What forces do molecular substances have

A

Intermolecular forces -usually weak

25
Q

What structure do giant covalent make

A

Large lattice

26
Q

What is diamond an allotrope of?

A

Carbon

27
Q

How do you boil/melt giant covalent structures?

A

-Bonds must be broken
-high heat to break strong covalent bonds

28
Q

Definition of giant covalent layered

A

infinite lattice of covalently bonded atoms in two dimensions only to form layers. The different layers are held together by intermolecular forces, and there are often delocalized electrons in between the layers

29
Q

What kind of properties does carbon have due to its delocalised electrons

A

-conductor of electricity
-low density due to spaces held by IM forces
-soft as layers can slide

30
Q

What are the two VSEPR theory rules

A

i) All σ-bonded electron pairs and all lone pairs arrange themselves as far apart in space as is possible. π-bonded electron pairs are excluded.
ii) Lone pairs repel more strongly than bonding pairs.
These two rules can be used to predict the shape of any covalent molecule or ion, and the angles between the bonds.

31
Q

2 electron pairs angle

A

180 (c—0—c)-linear

32
Q

Three electron pair angle

A

120 *-trigonal planar

33
Q

What is the bond angle and shape for Lone pair+ two bonding pairs?

A

-Bond angle is less than 109.5° but greater than 104°
-Bent

34
Q

What is the shape and bond angle of a molecule with 4 electron pairs?

A

109.5° (draw like trigonal planar with lone pair)
Dots -wedge -line=TETRAHEDRAL

35
Q

4 bonding pair but one a lone pair

A

Same structure of drawing but 109* =107 is smaller due to repulsion -TRIGONAL PYRAMIDAL

36
Q

5 electron pairs

A

Trigonal =120
Plus linear=90
=TRIGONAL BIPRYMIDAL

37
Q

6 electron pairs

A

90
OTRAHEDRAL
Two bonds outwards two sideways

38
Q

4 bonding pairs and 2 lone pars

A

Bonding pairs=90
Lone pair 180
Similar to octahedral but further repulsion from lone pair creating 180 bond angle between
SQAURE. PLANAR

39
Q

What is a temporary dipole

A

Electrons are in a constant state of motion when there is a surplus on one atom this creates the dipole creating VDW

40
Q

Induced dipole

A

VDW’s between two molecules

41
Q

What is needed for hydrogen bonding

A

-Hydrogen bonded to either N O F
-need a lone pair

42
Q

Why does ice have a low density?

A

H bonding Maxine’s space between molecules -open hexagonal structures

Chemistry (28 decks)

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