Shell Orbitals and periodic table

Question 1

What are electrons?

Answer 1

Negatively charged sub atomic particles that orbits the nucleus in shells

Question 2

What is the ground state of an electron

Answer 2

The orbital that they are present in when they aren’t excited

Question 3

What is the maximum number of electrons per energy level

Answer 3

2n^2

Question 4

Define an excited electron

Answer 4

An electron with a higher energy level than its ground state when it is given extra energy

Question 5

How do electrons become excited

Answer 5

When they are given energy- usually photons

Question 6

Define electron decay

Answer 6

The excited state is short lived and the electron returns to its ground statw

Question 7

How do electrons release ebergy

Answer 7

When electrons return to their ground state or lower energy level they release a photon with a specific energy eleven

Question 8

What is Bohr’s model

Answer 8

1) electrons orbit the nucleus
2) they orbit stably without radiating in discrete sets of distances called energy levels or shells
3) electrons can only gain/lose energy by absorbing or emitting energy
4) the energy of the orbit is related to its size

Question 9

What are the 4 orbital types

Answer 9

S, p ,d, f

Question 10

Describe the s orbital

Answer 10

• closest to the nucleus
• spherical
  -lowest energy
  Holds 2 electrons

Question 11

Describe the d orbital

Answer 11

• 4lobes that point in particular directions
• there are 5 orbitals
  -each orbital holds 2 electrons
  D orbitals hold 10 electrons in total

Question 12

Describe the p orbitals

Answer 12

• two lobes that point in particular directions
• has 3 orbitals
• each orbital hold a max of 2 electrons
• in total, p hold 6 electrons

Question 13

How do electrons fill up orbitals

Answer 13

• electrons fill the lowest energy levels first (Aufbau)

- degenerate orbitals are partially filled before orbitals are completely filled (Hund)

Question 14

Where is the S block on the periodic table

Answer 14

Group 1 and 2

Question 15

Where is the p block on the periodic table

Answer 15

Group 13-18

Question 16

Where is the d block on the periodic table

Answer 16

Group 3 -12

Question 17

Where is the f block on the periodic table

Answer 17

Group 6 and 7

Question 18

What happens to the atomic radius across a perios

Answer 18

Decreases bc more protons inc the nuclear charge an there are the same amount of shells and shielding so there are larger forces of attraction

Question 19

What happens to atomic radius down a group

Answer 19

Increases bc more shells are added so there are less forces of attraction between the nucleus and electrons

Question 20

Define cation

Answer 20

Positively charged metal ions

Question 21

Define anion

Answer 21

Negatively charged non metal ions

Question 22

Define a chemical bond

Answer 22

Forces that hold two or more atoms together and makes them function as a unit

Question 23

Define bond energy

Answer 23

The energy required to break a chemical bond

Question 24

Describe ionic bonding

Answer 24

• btw metal and non metal
  Complete transfer of electrons
• metals donate electrons while non metals accept electrons
• forms a lattice

Question 25

Describe a covalent bond

Answer 25

• Btw 2 non metal

- Sharing of electrons

Question 26

Describe a polar covalent bond

Answer 26

• btw 2 non metals

- unequal sharing of electrons bc of electronegativity

Question 27

What is the octet rule

Answer 27

Metals and non metals form ions in order to achieve the electronic configuration of a noble gas

Question 28

Define ionisation energies

Answer 28

The amount of energy required to remove an electron from 1 mole of gaseous atoms

Question 29

What happens to ionisation energies across a perios

Answer 29

Increases bc a higher nuclear charge and same amount of shielding

Question 30

What happens to ionisation energies down a group

Answer 30

Decreases bc valence electrons have less forces of attraction with the nucleus

Question 31

Define electronegativity

Answer 31

The power of an atom to attract the electron density on a covalent bond towards itself

Question 32

What is the most electronegative atom

Answer 32

Fluorine