Bonding

Question 1

Ionic bonding involves the transfer of electrons from a _____element to a ______element

Answer 1

Ionic bonding involves the transfer of electrons from a metallic element to a non-metallic element

Question 2

which atoms gain electrons and which lose it

Answer 2

metals lose e-
non metals gain e-

Question 3

what are the electron configurations the same as when they are ions

Answer 3

noble gases

Question 4

diagram for ion dot cross

Answer 4

brackets
charge at top leaft
outer shell e-
dots for other ion

Question 5

ionic bond

Answer 5

electrostatic attraction between oppositely charged ions

strong so requires lots of energy to overcome

Question 6

structure

Answer 6

giant ionic lattice regular repeating pattern
therefore attraction is occurring in all directions
final lattice is neutral

Question 7

ionic radius

Answer 7

measure of the size of an ion

Question 8

ionic radii pattern

Answer 8

increases with increasing negative charge

therefore decreases with increasing positive charge

Question 9

negative ions formed by gaining electrons affect on ionic radius

Answer 9

outermost e- are further away so therefore only held weakly to the nucleus , increasing ionic radius

Question 10

positive ions formed byy losing e- affectonnuclearchargeandionicradius

Answer 10

nuclear charge stays same but fewer e- to undergo a greater electrostatic force of attraction which decreases ionic radius

Question 11

isoelectronic

Answer 11

ions with the same electronic configuration yet a different number of protons

leading to different sizes of ions

Question 12

type of lattice formed depends on

Answer 12

sizes of the positive and negative ions which are arranged in an alternating fashion

Question 13

high melting point of ionic

Answer 13

strong electrostatic attraction between oppositely charged ions which requires lots of energy to overcome

Question 14

the greater the ionic charge

Answer 14

the greater the melting point

Question 15

electrical conductivity of ionic

Answer 15

no free flowing charged particles which would usually carry the charge between uions.
can conduct in a solution or molten as ions can move and carry charge

Question 16

solubility ionic

Answer 16

are soluble as are polar molecules (when put in polar solution)
when in solution the negative ion in compund bonds to the positive in solution and the opposite.

solubility depends on the relative strength of electrostatic forces of attraction within lattice

Question 17

evidence for existence of ions

Answer 17

electrolysis

Question 18

copper chromate in electrolysis

Answer 18

blue at negative elctrode cu at - which are blue

yellow at positive electrode CrO4 at positive and their ions are yellow

Question 19

bond energy

Answer 19

energy required to break one mole of a particular covalent bond in gaseous state

Question 20

bond length

Answer 20

inter-nuclear distance between two covelantly bonded atoms

Question 21

increasednumberofbondsaffect on bond length (eg c=c)

Answer 21

increased force of attraction by shared electrons and positive nuclei decreases the bond length

therefore the more bonds eg c=c the shorter the bond

Question 22

bond lengthaffect on bond energy

Answer 22

energy required to break one mole of a covelant bond increases with decreasing bond length

eg. c=c is higher bond energy than c-c

Question 23

simple covelant properties and reason

Answer 23

weak intermolecular forces

require little energy to overcome

Question 24

diamond properties and reason

Answer 24

very hard and high melting point

lots of strong covelant bonds

arranged in a tetrehedral structure - difficulpt to break

requires lots of energy to overcome

Question 25

graphite properties and reason

Answer 25

each carbon atom bonded to 3 others

has delocalised electrons

free electrons migrate across layers and carry charge and electricity

contaies layers connected by london forces which can slide so it is malleable

Question 26

metallic bonding

Answer 26

electrostatic attraction between positive metal ions and a sea of delocalised electrons

positive charges repel, keeping them arranged in a lattice

delocalised electrons can carry charge