bonding

Question 1

define ionic bonding

Answer 1

the electrostatic forces of attraction between oppositely charged ions occurring in all directions in a giant ionic lattice.

Question 2

how is an ionic bond formed?

Answer 2

metals lose outer electrons to form positive ions (cations); non metals gain electrons forming negatively charged ions (anions)

Question 3

what is the purpose of atoms forming ions?

Answer 3

to obtain a full outer shell of electrons; the electron configuration of a noble gas therefore

Question 4

describe the electrostatic forces of attraction

Answer 4

they are really strong and act in all directions

Question 5

list some common ionic compounds

Answer 5

sodium chloride, magnesium oxide, barium sulfate, lithium carbonate, rubidium bromide.

Question 6

describe the structure of an ionic compound.

Answer 6

the oppositely charged ion being held by really strong electrostatic forces of attraction (taking lots of energy to overcome) form a lattice structure in the form of an evenly distributed crystalline. it is a regular pattern. each ion is attracted to all of the oppositely charged ions around it

Question 7

what charge does the overall lattice have and why?

Answer 7

overall electrically neutral because the positive charges cancel negatives therefore

Question 8

state the effect of melting and boiling points on ionic compounds and why

Answer 8

melting and boiling points are high because the giant ionic lattice is being held by strong electrostatic forces of attraction which take a lot of energy to overcome

Question 9

why do different compounds have different melting points and what does the effect have overall?

Answer 9

different ionic compounds can be having different melting and boiling points due to the ions having stronger charges. strong charge means greater attraction between the ions
for example, the charges of magnesium oxide are 2+ and 2- which are larger compared to the charges of sodium chloride, are 1+ and 1-. therefore, there is greater attraction between the magnesium and oxide ion compared to the sodium and chloride ion.

Question 10

state the effect of ionic compounds being able to dissolve in water

Answer 10

water molecules are polar and they surround the compound. water has a positive and negative charge and can therefore be pulling the ions but the from lattice, causing dissolving

Question 11

what effect does the charge of an ion have on solubility?

Answer 11

charges larger means solubility decreases because water molecules cannot overcome the electrostatic forces of attraction

Question 12

what effect does the ability to conduct electricity have on ion?

Answer 12

if the compound is either molten or dissolved it can conduct electricity because the ion can therefore carry a charge compared to when theyre being held by electrostatic forces

Question 13

define covalent bonding

Answer 13

A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. (non metals)

Question 14

explain why covalent bonds are strong

Answer 14

there are electrostatic forces of attraction between the nuclei of both atoms and bonding electrons of their outer shells so

Question 15

state some examples of covalent bonds

Answer 15

Cl2, CH4, CO2, H2O, HCl

Question 16

what types of bonds can atoms also be forming?

Answer 16

double and triple covalent bonds which contain multiple shared pairs of electrons therefore

Question 17

what are the types of covalent structures?

Answer 17

simple molecular substances - gases and liquids and giant covalent (macromolecular) - solids

Question 18

what is the melting point of a simple molecular substance and why?

Answer 18

low because even if the bonds are strong due to covalent bonds, the layers between the molecules are held weakly by intermolecular forces

Question 19

what is the solubility of a simple molecular substance?

Answer 19

low

Question 20

can simple molecular substances conduct electricity + why?

Answer 20

no even if the substances are molten or dissolved. there are no charged particles for example ion

Question 21

state some examples of giant covalent substances

Answer 21

diamond graphite and silicon dioxide

Question 22

describe the structure of diamond

Answer 22

diamond is the hardest substance and is made of carbon atoms and each carbon atoms is covalently bonded to about therefore four other carbon atoms. the atoms are arranged in a tetrahedral shape.

Question 23

explain why diamond is the hardest substance

Answer 23

strong covalent bonds and therefore used in diamond tipped drills and saws

Question 24

why does diamond have a high melting point?

Answer 24

the strong covalent bonds holding the structure together take loads of energy to overcome when heated