Unit 1

Question 1

wt is ionisation energy

Answer 1

the energy needed to remove and electron from an atom or ion

Question 2

how does the postition of an electron within quantum shells affect its ionisaiton energy

Answer 2

electrons in outer shells have lower ionizaiton energy cuz they r father from the nucleus and sheilded by inner electrons, making them easier to remove

Question 3

wt happens to the ionisation energy as u move down a grp

Answer 3

decreases

Question 4

primary function of a mass spectromter

Answer 4

meauss the mass-to-charge ratio of ions

Question 5

how does atomic radisu relate to ionisaiton energy trends accross periods and grps

Answer 5

ionization energy decreases with larger atomic radius (down grps) and increases with smaller raidus (across periods)

Question 6

relative isotpic mass meaning

Answer 6

mass of an isotope relative to 1/12 the mass of C-12

Question 7

why does neon hve thre highest first ionisation energy amoung the elements in period 2

Answer 7

cuz it has a full valence shell. this make sis very stable, needing more energy to remove an electron

Question 8

wt is the relationship between mass-to-charge ratio and ion defection in a mass spectrometeri

Answer 8

ions with lower mass-to-charge ratios delfect more in a mass spectromteter cuz they r lighter

Question 9

wt info can be taken from the peaks in a mass spectrium

Answer 9

mass-to-charge ratio
relative abundance of ions
isotpic abundance
molecular weight

Question 10

how do u determine the relative molecular mass of diatomic molecules using mass spectrometery

Answer 10

mass spec ionizes molecules, seperates ions by mass-to-charge ratio. for diatomoic, the (M+) peak indicated relative molecular mass.

Question 11

wt r the 4 factors that influecne ionization energies

Answer 11

nuclear charge
atomic radius
electron shelding
subshell stabiloty

Question 12

describe the process of the mass spectrometer and the parts

Answer 12

https://www.google.com/url?sa=i&url=https%3A%2F%2Fmicrobenotes.com%2Fmass-spectrometry-ms-principle-working-instrumentation-steps-applications%2F&psig=AOvVaw1F56noX8RAKb1_UYk5nx10&ust=1743125566187000&source=images&cd=vfe&opi=89978449&ved=0CBQQjRxqFwoTCJjU6PSOqYwDFQAAAAAdAAAAABAJ

Question 13

explain y the ram of manyn elements arent whole numbers

Answer 13

Most elements exist as a mixture of isotope so Each isotope has a different percentage abundance

Question 14

wt is the electronic configuration template

Answer 14

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10

Question 15

describe s orbtial

Answer 15

Spherical in shape.
Can hold a maximum of 2 electrons.

Question 16

describe p orbital

Answer 16

Dumbbell-shaped.

Each p-orbital holds 2 electrons
so a full set holds 6 electrons.

Question 17

describe d orbital

Answer 17

cloverleaf-shaped
Each d-orbital holds 2 electrons, so a full set holds 10 electrons.

Question 18

show second ionisation energy of A

Answer 18

A+(g) —–> A2+(g) + e

Question 19

explain the anormali of B in the ionisagion energies plot

Answer 19

although the nucleuar chage of B is greater than Be, the outer electron of boron has more energy since it is in a 2p orbital as opposed to the 2s orbital for Be, so the energy needed to remove 2p electron in boron is less than the energy needed to remove a 2s electrno fron Be

Question 20

describe the nature of ionic bonidng

Answer 20

ionic bonding occurs in solid material consisting of a regular array of oppositely charged ions extending thruout agiant lattice network

Question 21

why does the size of the ion affect the strength of the ionic bond

Answer 21

cuz it determineshow closely packed the ions r in the lattice

Question 22

wt happenes to the ionic radi as the no of protons increases

Answer 22

it decreases

Question 23

how is polariation increaed of catiosn and anions

Answer 23

cation- high charge ad small size of the cation
anion- high charge and large size of the anion

Question 24

charge densitiy eqaution

Answer 24

charge/r2

Question 25

describe the formation of covalent bonds

Answer 25

a covalent bond forms between 2 atoms when a single orbital from one atom overlaps which another orbtial which also has a singole elctron. the two electrons in the area of overlap r the bonding electrons

Question 26

wt r the 3 ways in whih the covalent bonds can overlap and tate if they r a sigma or pi bond

Answer 26

end on overlap of 2 s orbital (sigma) end on overlap of 2 p orbitals (sigma) sideways overlap of 2 p orbitals (pi)

Question 27

explain the relationship between bond length and bond strength in coalent bonds

Answer 27

shorter the bond, greater the stregnth. this is a result of increase in electrostatic attraction between the two nuclei an the electrons in the overlaping atomic orbitals

Question 28

why does electrongativity decrease down a grp

Answer 28

Atomic radius increases More electron shielding → Inner electron shells repel outer electrons, reducing nuclear attraction. Weaker nuclear attraction

Question 29

why does electrongativity increase across a period

Answer 29

Nuclear charge increases Atomic radius decreases Shielding remains relatively constant → No extra inner shells are added.

Question 30

how is a dative covalent bond formed

Answer 30

its formed when an empty pair of ortbia of one atoms overlaps with an ortbial containign a lone of pair eletrons

Question 31

draw the metal lattice strcytre

Answer 31

https://images.app.goo.gl/2qT7cicW7MjqjNQh6

Question 32

how is cracking done and wt is the catalyst

Answer 32

its done by passing the hydrocarbons thru a heated catalyst (zeoltide) . this causes larger molecules to break into smller ones.

Question 33

wt is reforming used for and wt is the catalyst used

Answer 33

used to convert straight chain alkanes into branched chin alkanes and cyclic hydrocarbons by heating them with a catalyst (platinum)

Question 34

wt happens when some atoms of sulfur isnt removed f rom frational distilation, cracking or reforming process

Answer 34

during the combustion of alkanes, these sulfur atoms form sulfur dioxide gas and then can react in the atmoshphere to form sulfur trioxide gas

Question 35

wt is carbon neutral

Answer 35

Carbon neutral means balancing the amount of carbon dioxide released with the amount removed from the atmosphere, so the net emissions are zero.

Question 36

wt happens in the substituion reaction of alkanes

Answer 36

a halogen takes the place of the hydrogen atom

Question 37

describe the formation of igma bonds

Answer 37

A sigma bond is formed by the direct, head-on overlap of orbitals along the internuclear axis. This overlap results in a high electron density between the two nuclei, creating a strong electrostatic attraction that holds the atoms together. Sigma bonds can form through the overlap of two s orbitals, an s and a p orbital, or two p orbitals.

Question 38

describe the formation of pi bons

Answer 38

A pi bond is formed by the sideways overlap of adjacent p orbitals above and below the internuclear axis. This type of overlap creates a region of electron density located above and below the bonded atoms, . Unlike sigma bonds, pi bonds restrict rotation around the bond axis due to the electron density being spread over two regions

Question 39

define strucular isomers

Answer 39

compounds with the same molecular foeula but diff struuctral formula