Bonding

?
What are the three types of bonds?
Ionic, Metallic and Covalent
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Describe ionic bonding?
Occurs between non-metals and metals. An electrostatic attraction between pos & neg ions. Structure = lattice
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Properties of ionic compounds?
Solids at room temp. Giant structures and high mp. Conduct electricity when molten/dissolved.
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What is a covalent bond?
Pair of non-metals. A shared pair of electrons.
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What is Dative Covalent bonding?
The atom that accepts electron pair in electron deficient. The atom that is donating the atom and has a pair not being used is called a lone pair. E.g. Ammonia. (one atom provides both of the shared electrons)
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Describe metallic bonding?
A lattice of positive ions with a sea of delocalised electrons.
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Properties of metals?
Good conductors of electricity – delocalised electrons can move. Strength of metals – depends on size (smaller the ion, the closer they are to the positive nucleus) and charge of ion (greater charge = greater number of delocalised electrons). Malleab
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Define electronegativity?
Electronegativity is the power of an atom to attract the electron density in a covalent bond towards itself.
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What does electronegativity depend on?
Nuclear charge, Distance between the nucleus and the outer shell of electrons, Shielding of the nuclear charge by electrons in inner shells.
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What are the trends in electronegativity?
Going across a period the electronegativity increases. The nuclear charge increases.
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What are covalent bonds between two atoms that are different called?
Polar – the greater the difference in electronegativity, the more polar the covalent bond is.
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What are the three types of intermolecular forces?
Van der Waals – act between all atoms and molecules (weakest). Dipole-dipole – act only between certain types of molecules. Hydrogen bonding – acts only between certain types of molecules (strongest).
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Describe dipole-dipole forces?
Acts between molecules that have a permanent dipole.
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What are van der Waals forces?
All atoms and molecules are made up of positive and negative charges. These charges produce very weak electrostatic attractions between all atoms and molecules.
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What is hydrogen bonding?
Consists of hydrogen atom ‘sandwiched’ between two very electronegative atoms. Stronger because the oxygen atoms in water have lone pairs of electrons.
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When do hydrogen bonds form?
Oxygen, nitrogen and fluorine.
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What is the electron pair repulsion theory?
Each pair of electrons around an atom will repel all other electron pairs. The pairs of electrons will therefore take up positions as far apart as possible to minimise repulsion.
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Draw the structure for ammonia
Trigonal pyramid. 107
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Draw the structure for water
Non-linear.104.5
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Draw the structure for carbon dioxide
Linear
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What are induced dipoles?
Temporary dipoles created in all atoms and molecules due to the movement of electrons. All atoms and molecules
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Permanent dipoles - how do you know if a covalent bond is polar?
Electrons are shared unequally between atoms being bonded. Permanent dipole attractions are stronger.
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Effects of hydrogen bonding?
Higher mp & bp. Greater viscosity and solubility in water. Specific molecular shape.
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What is the order of attraction between lp-lp, lp-bp and bp-bp
lp-lp > lp-bp > bp-bp
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Draw the shape of two pairs of electrons and give the name and bond angle
Linear.
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Draw the shape for three pairs of electrons and name the shape and bond angle.
Trigonal planar. 120
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Draw the shape for four pairs of electrons and name the shape and bond angle.
Tetrahedral. 109.5
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Draw the shape for five pairs of electrons and name the shape and bond angle.
Trigonal Bipyramid. 90 and 120
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Draw the shape for six pairs of electrons and name the shape and bond angle.
Octahedral. 90
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Draw the shape for four bonds and one lone pair.
Seesaw. 102 and 86.5
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Draw the structure for 3 bonding pairs and 2 lone pairs.
T-shape. 87.5
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Draw the structure for 5 bp and 1 lp.
Square pyramid. 90
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Draw the shape for 4bp amd 2lp
Square planar. 90
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Other cards in this set

Card 2

Front

Describe ionic bonding?

Back

Occurs between non-metals and metals. An electrostatic attraction between pos & neg ions. Structure = lattice

Card 3

Front

Properties of ionic compounds?

Back

Preview of the front of card 3

Card 4

Front

What is a covalent bond?

Back

Preview of the front of card 4

Card 5

Front

What is Dative Covalent bonding?

Back

Preview of the front of card 5
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