Small Important Questions Flashcards

1
Q

Name the sub — atomic particles of an atom.

A

Proton
Neutron
Electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Name the scientist who formulated the atomic structure

A

John Dalton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the e/m ratio of an electron

A

according to Thomson’s experiment 1.76x10^3, every gram of electron carries the following charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

name of the scientist who first gave the atomic model

A

JJ Thomson

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is an isotope

A

atoms with the same atomic number but different mass number are called isotopes, they have similar chemical properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what are isobars

A

atoms with the same mass number but different atomic numbers are called isobard they have different chemical properties but same physical properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

define photoelectric effect

A

when the surface of alkali metals like potassium and calcium emit electrons when a beam of light with high frequency is projected on them is called photoelectric effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is an atomic number?

A

Atomic number is the measure of the number of protons which is present in
the nucleus of an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is a mass number?

A

Mass number of an element is the sum of the number of protons and
neutrons present in the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How does the intensity of light affect photoelectrons?

A

The number of electrons ejected and kinetic energy associated with them is
directly proportional to the intensity of light projected towards the metal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Quantum Numbers

A

Quantum numbers are 4 different QN which together lets us know the probable location of an electron in orbit.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Principle quantum number

A

this quantum number lets us know the size of the atom; it is denoted by “N” where n is the shell in which the electron is present. Bigger the number further away the electron is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Azimuthal Quantum Number

A

It represents the subshell in which electrons belong to, it also gives us the shape of the orbitals. Azimuthal quantum number is denoted by the letter “l” in which l = (n-1).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Magnetic Quantum Number

A

This QN gives us all the possible orbitals/orientations possible for a specific in a subshell. It is represented my ML and ML = -L 0 +L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Spin Quantum Number

A

This gives us the information of spin direction of the electron. These possible values are +1/2 and -1/2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Bond Order

A

Its defined as half of the difference between the no of electrons present in the bonding electrons and anti-bonding electrons (BO = ½ (ES1 – ES2))

17
Q

Hund’s rule of maximum multiplicity

A

All the pairing of electrons will only take place if all the orbitals are occupied with a single electron

18
Q

Paulis exclusion principle

A

No 2 elements can have the same value for all 3 quantum numbers

19
Q

Aufbau principle of maximum multiplicity

A

The elements are arranged in the orbitals in the increasing order of their energy

20
Q

Molecular orbital theory

A

each atom tends to combine together and form molecular orbitals.

21
Q

Valence bond theory

A

Those atoms which have opposite spin electrons overlap with each other to form a bond between the 2 atoms, as this overlapping increases the stability of the bond also increases

22
Q

Polarity of bonds

A

the existence of positive and negative charged electrons are called polarity of bonds

23
Q

Dipole Movement

A

dipole movement is defined as the measure of polarity of a bond

24
Q

Bohr’s Atom model

A

the model which can represent each shell in which the electrons are present are called bohr’s atomic model

25
Q

Heisenberg Uncertainty principle

A

It states that it is impossible to determine the velocity and position of an microparticle simultaneously

26
Q

Demerits Bohr’s model

A
  • Couldn’t explain the dine details of hydrogen spectrum
  • Couldn’t explain the spectrum of atom other than hydrogen
  • Couldn’t explain the formation of molecules by chemical bonding
  • Couldn’t explain Zeeman and stark effect
27
Q

iso electron species

A

the species (different elements) with the same number of electrons is called iso electron species