Chem bonding and structures of matter

Question 1

Bonding present in a Ionic Compound?

Answer 1

Strong electrostatic forces of attraction hold positive ions and negative ions together to form a giant lattice structure

mistake: no ionic crystal

Question 2

Structure of Ionic bonds

Answer 2

Giant Ionic Crystal Lattice Structure

Question 3

Volatility of a ionic compound

Answer 3

High melting and boiling point.

Large amount of energy needed to overcome strong electrostatic forces of attraction present between ions in the giant lattice structure

Question 4

State of ionic compounds

Answer 4

Solids at room temperature

Why? high volatility

Question 5

Solubility of ionic compounds

Answer 5

Soluble in water (polar solvents) , but not in organic compounds.

Type of attraction in ionic compounds similar to that of water, but not in organic solvents.

Question 6

Electrical Conductivity of ionic compound 💕

Answer 6

In solid:
Ions are held together in fixed position in a giant ionic crystal lattice structure

In liquid:
Strong electrostatic forces of attraction (BONDS) between ions are broken down (completely), ions can move freely (mobile) and conduct electricity.

Question 7

Bonds of a covalent compound (SMS)

Answer 7

Simple discrete molecules held together by strong electrostatic forces of attraction between positively-charged nucleus and negatively-charged shared pair of electrons

*common mistake: muss diff btw gms i.e simple discrete molecules NOT atoms

Question 8

Bonds present btw atoms vs bonds present btw molecule (SMS)

Answer 8

Each atom is held together by strong electrostatic forces of attraction&raquo_space; large amount of energy needed to overcome

Note: higher bp tk do this (i.e atomization)

Question 9

structure of the covalent compounds

Answer 9

simple molecular structure

Question 10

Volatility for Covalent Compound (SMS)

Answer 10

Small amount of energy is needed to overcome weak intermolecular forces of attraction btw molecules, thus, there there is a lower bp/mp

Question 11

state of the covalent compound at r.t.p (SMS)

Answer 11

exist as liquid/gas at r.t.p&raquo_space;low mp/bp

Question 12

Solubility of Covalent Compounds (SMS)

Answer 12

Soluble in organic solvents and NOT polar solvents

Question 13

Electrical conductivity of Simple Molecular Structure

Answer 13

Cannot conduct electricity in ANY STATE as SMS made of molecules which do not carry any charge, thus cannot conduct electricity due to the absence of mobile CHARGE carriers.

*mistake: charge

Question 14

Bonding present in Covalent Compound (GMS)

Answer 14

EXTENSIVE NETWORK OF atoms held together by strong electrostatic forces of attraction btw positively charged nucleus and negatively-charged shared pair of electrons.

Question 15

Volatility of Covalent Compound (GMS)

Answer 15

Large amount of energy needed to break apart strong efoa btw positively charged electrons and negatively charged shared pair of electrons

*just covalent bonds can too

Question 16

Structure of a Giant Molecular Structure

Answer 16

Giant Molecular Structure

1. Tetrahedrial Structure

Large nom of strong cov bonds present throughout extensive network structure
(each C atom bonded to 4 other C atom)
Diamond, Silicon Dioxide
2. Hexonigal Structure

Layers of atoms slip and slide over one another due to presence of weak IMFOA

Graphite

(each c atom bonded to 3 other C atoms)

Question 17

MELTING point of graphite VS diamond

Answer 17

diamond has tetrahedrial structure. large no. of strong cov bonds throughout large extensive network structure. Greater amoumt of energy needed to overcome cov bonds

graphite has a hexonigal structure, presence of weak imfoa btw layers of carbon atom, this causes CARBON atoms to slide over one another
Less energy needed to overcome weak IMFOA

Question 18

State and Texture of GMS

Answer 18

Solid at r.t.p

1. Graphite : layers of carbon atoms slip and slide over one another&raquo_space; soft and slippery
2. Diamond : large no. of strong cov bonds present throughout extensive network structure》》 rigid》》hard and strong

Question 19

Solubility of GMS

Answer 19

Insoluble in every solvent

Question 20

Electrical Conductivity of GMS

Answer 20

1. Diamond (tetrahedrial)

each C atom bond to 4 other C atoms via via single c-c cov bond, thus all of valence electrons involved in bonding, unable to conduct electricity due to absence of mobile charge carriers

Graphite (hexonigal) :

Each C atom is bondes to 3 other C atoms via ssingle c-c cov bonds, presence of one valence electron per carbon atom, thus able to conduct elec along the layers of graphite.

note: each layer=1 molecule

Question 21

Bonding in a metal compound

Answer 21

Strong efoa btw positively charged metal atoms and negatively charged sea of delocalized electrons.

Question 22

Structure of metal compounds

Answer 22

Giant Metallic Lattice Structure

Question 23

Volatility of metal compounds

Answer 23

Large amount of energy needed to break strong efoa btw + charged metal atoms (cations) and - charged sea of delocalized electrons (metallic bonds)

Question 24

Solubility of metal compounds

Answer 24

Insoluble in any solvent

Question 25

Electrical conductivity of metal compounds

Answer 25

can conduct elec in all states due to presencd delocalized electrons which act as mobile charge carriers to conduct elec from + terminal of source and move btw the catio s in the metallic structure

Question 26

Malleability (bends easily)and Ductility (easily pulled thru wires) of metallic compounds

Answer 26

When valence elec of an atom delocalize, dont belong to any atom> metal atoms are similarly sized and arranged in regular layers. if force applied = layer of metal atoms slide thru each other (thru delocalized e-) w/o disrupting the metal lattice

Question 27

What is electronegativity?

Answer 27

Measure of the tendency of an atom to attract a bonding pair of electrons

Question 28

What affects erectronegativity?

Answer 28

Higher number of proton in nucleus: stronger electronegativity

Smaller distance of shared electrons from nucleus : stronger electronegativity

little shielding effect by inner electrons: stronger electronegativity

Question 29

What if equal electronegativity?

Answer 29

Same tendency to attract bonding pair of electrons: found ave-halfway btw 2 atoms

only for same element: diatomic( ie. H2 02)

Pure covalent bond

Question 30

It B is slightly more electronegative than A

Answer 30

Element has more than its fair share of electron density : more electronegative

Pulls electron towards nucleus has slightly negative charge:

Other elements is much less electronegative: cannot hold onto electrons as well: slightly positive charge

Electron pair dragged over to b

Question 31

What affects bonding in ionic compound

Answer 31

1. Size of ion
   Size of ion decreases: ionic radii decreases: decrease strength of electrostatic forces attraction between positive and negative ions: less energy needed to overcome strong ionic bonds: decrease melting point
2. lonic charge
   Electrostatic forces of attraction between decrease energy positive ion and negative ions decreased : decrease energy needed to overcome strong ionic bonds present btw ions in the ionic compound= decrease melting boiling point

Question 32

What affects bonding in a covalent substances

Answer 32

Bond Size/ molecule:
bonding btw molecules- intermolecular forces of attraction
Increase bond size= stronger intermolecular forces of attraction btw molecules = more energy needed to overcome imfoa= higher bond/map

Bond length:
Bonding btw each atom in a molecule
CoV bonds
If no. Of electron shells decrease= decrease distance btw positively charged nucleus and negatively chaired shared pair of electrons= stronger cov bonds = more energy needed

Bond energy:
Atoms of a molecule
CoV bonds
Greater bond energy= stronger CoV bonds= increase energy needed

Question 33

What is bond length

Answer 33

Average distance btw nuclei of 2 CoV bonded atoms of a molecule

Question 34

What is bond energy.?

Answer 34

Amount of energy needed to overcome bonds btw one mol of CoV bonded gas

Vibrate until atoms are energetic enough to overcome strong CoV bonds btw positively charged nuclei and negatively charged shared pair of electrons

Question 35

What affects bonding-in a metallic compound.

Answer 35

1. No. Of valence electrons
   Increase number of valence electrons = no. Of valence electrons lost to form cations = increase no of delocalized electrons in the metallic lattice structure = more energy needed to overcome strong electrostatic forces of attraction btw positively charged metal cation and sea of delocalized electrons ( METALLIC BONDS) = higher mp/ bp
2. Electron shells
   If no.of electron shells increase= distance btw positively charged metal cation and sea of delocalized electrons increase= decrease strength of metallic bonds = less energy needed to overcome efoa btw + charged cation and - charged sea of delocalized electrons ( METALLIC BONDS) = higher mp/ bp