1st SEMESTER

Question 1

Define electromagnetic spectrum.

Answer 1

Range of frequencies based on wavelength.

Question 2

Gamma Particles

Answer 2

Type of radioactive particle that has neither mass or electric charge (neutrons).

Question 3

He discovered protons.

Answer 3

Eugene Goldstein

Question 4

Maximum electrons per energy level.

Answer 4

𝑛2

Question 5

Atomic number is equal to number of?

Answer 5

Protons

Question 6

He discovered that electrons orbit the nucleus and that they jump to lower-energy orbit and emits energy as radiation.

Answer 6

Neils Bohr

Question 7

Explain Cathode Ray Experiment.

Answer 7

Cathode rays travel in a straight line. Due to the negatively charged particle inside the tube. They are repelled and attracted to the anode (+) bending the rays leading to the discovery of a negative charge in an atom called cathode (electrons).

Question 8

Sublevels of M energy level.

Answer 8

s, p, d

Question 9

_____________ dependent on the number of atomic orbitals.

Answer 9

Ionization Energy

Question 10

Discovered the nucleus through the famous goild foil-alpha particle experiment.

Answer 10

Ernest Rutherford

Question 11

Charged particle.

Answer 11

Ion

Question 12

He said that matter consist of tiny indivisible particles and called it “atomos”.

Answer 12

Democritus

Question 13

Lewis-Chemical Formula of MgCl₂

Answer 13

__________

Question 14

Shapes of the different sublevels.

Answer 14

s- spherical, p- dumbbell, d,f- spherical and dumbbell.

Question 15

Define IONIC bonds.

Answer 15

Characterized by gaining or losing of electrons which happens between charged particles.

Question 16

When an atom gains electron/s, it acquires a __________.

Answer 16

Negative Charge

Question 17

Polarity depends on the atom’s?

Answer 17

Electronegativity

Question 18

It is the unequal sharing of electrons.

Answer 18

Polar Covalent Bonds

Question 19

Why does 4s lies between 3p and 3d energy level?

Answer 19

4s has lower energy than 3d but higher than 3p.

Question 20

Bond strength

Answer 20

Amount of energy needed to break or make a bond. The strength at which a chemical bond holds two atoms together.

Question 21

Covalent Bonds.

Answer 21

Characterized as the sharing of electron pair between atoms. Overlapping of orbitals result this type of bond.

Question 22

Equal sharing of electrons between gas atoms.

Answer 22

Non polar covalent bonds.

Question 23

He discovered electrons and proposed the “Plum Pudding model”.

Answer 23

Joseph John Thomson

Question 24

Formed by head on overlapping of atomic orbitals.

Answer 24

Sigma (σ) bonds

Question 25

Postulates of Thomson.

Answer 25

1. Elements consist of indivisible small particles called atoms. 2. Atoms of the same elements are identical. 3. Atoms can neither be created nor destroyed. 4. Compound elements are formed when atoms of different elements join to form “Compound atoms”).

Question 26

Define Molecular Orbital.

Answer 26

It is formed when atomic orbital of one atom overlaps with an atomic orbitals of the other atom to form new orbitals.

Question 27

Possible overlaps of sigma bond.

Answer 27

Between two s orbitals, between one s orbital and one p orbital, and between two p orbitals.

Question 28

Bond order is determined by?

Answer 28

The number of shared electron pairs.

Question 29

Number of orbitals for each sublevel.

Answer 29

S-one, p-three, d-five, and f-seven.

Question 30

Differentiate alpa and beta particles.

Answer 30

Alpha particles (protons) are positively charged radioactive particles which moves slower and is denser than beta particles. Beta particles (electrons) are negatively charge radioactive particles that is faster and less denser than alpha particles.

Question 31

Mass number.

Answer 31

Equal to the sum of the number of protons (+) and neutrons (⁰).

Question 32

What are the atom’s energy level according to Neils Bohr?

Answer 32

(k) n=1 (L) n=2 (m) n=3 (n) n=4

Question 33

How does an electron maintain its position on the orbitals of an atom?

Answer 33

The tendency of the electrons (-) is to move fast to counteract their attraction towards the nucleus.

Question 34

Show the lewis structure of SO₄^-2

Answer 34

_________________

Question 35

Show the lewis structure of PO₄^-3

Answer 35

_________________