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Electronic configuration Flashcards

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1
Q

Mass of proton,neutron & which is heavier?

A

1 amu
Neutron is slightly heavier

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2
Q

Atom has many_____

A

empty space

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3
Q

Function of neutrons

A

hold the positively charged protons in the nucleus

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4
Q

A
X
Z Explain the symbols.

A

A=mass number (number of protons + neutrons)

Z=atomic number (Numberof protons & electrons)

X=element

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5
Q

How can isotope of elemnet exist?

A

The same atomic number but different mass number (Same number of protons but different neutrons numbers)

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6
Q

Is physical and chemical properties are same for isotopes?

A

Isotopes have same chemical properties (Reactivity,etc)
but have different physical properties such as melting and boliling point,density and gaseous diffusion

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7
Q

How to find the avrage atomic mass of elements which have isotopes?

A

Relative atomic mass= total mass/ number of atoms

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8
Q

Whan a chemical reaction occurs,what is the number that change?
a.proton b.neutron c.electrons

A

Eletrons

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9
Q

Sodium atoms are very reactive and gives off heat when dissolved in water, we are eating common salt daily, why isn’t it dangerous to human bodies?

A

Bcuz we are eating sodium ion Na+ ——> which does not have outer electrons——> not reactive

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10
Q

Most nutrients elements in food are present in the form of ions.The calcium ion Ca2+ is essential for healthy teeth and bones.Identify the sub-atomic particles present in the ions.

A

40 Ca2+
Number of protons+neutrons=40
Number of protons=20
Number of electrons=20-2=18

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11
Q

Identify the species with 19 protons,20 neutrons and 18 electrons.

A

Potassium cation

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12
Q

Although the mass number of carbon is 12, the relative atomic mass measured by spectrometer is slightly larger, why?

A

Bcuz of the occurrence of carbon12 and carbon 13; isotopes

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13
Q

What is the same for an atom of phosphorus-26 and an atom of phosphorus-27?
a)atomic number and mass number
b)Number of protons and electrons
c)Number of neutrons and electrons
d)Number of protons and neutrons

A

b)Number of protons and electrons

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14
Q

How is the frequency and wavelength proportional to?

A

Inversely proportional
v = fλ

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15
Q

How does the element release energy?

A

When an atom absorbs energy, electrons move into an orbit or higher energy level from the nucleus———> excited state====> unstable and falls back into the ground state/ the energy the electrons give off when it falls to the lower levels is one photon in the form of electromagnetic radiation.

The energy is proportional to the frequency of the radiation*

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16
Q

How wavelength,frequency & energy relate to?

A

Wavelength and frequency are inversely proportional.
(shorter wavelength—-higher frequency)

Frequency and energy are directly proportiona.
(High frequency—-high energy released)

Therefore,wavelength and energy are inversely proportional.
(Shorter wavelength—–higher frequency—-higher energy)

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17
Q

Decribe electromagnetic spectrum with shorter to longer wavelength.

A

Gamma ray—X rays—UV—Visible light—IR—Microwaves—Radiowaves

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18
Q

Which electromagentic radiation have shortest wavelength?

A

Gamma rays

(Shortest wavelegth,Highest frequency,highest energy)

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19
Q

Decribe electromagnetic spectrum with higher to lower frequency. (higher to lower energy)

A

Gamma ray—X rays—UV—Visible light—IR—Microwaves—Radiowaves

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20
Q

Which electromagentic radiation have longest wavelength?

A

Radio waves
(Longest wavelegth,lowest frequency,Lowest energy)

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21
Q

What is the wavelegth of gamma rays?

A

10^-6 nm

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22
Q

What is the wavelength of radio waves?

A

10^8 nm

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23
Q

What is the wavelength range of visible light spectrum?

A

4 x 10^-7 to 7 x 10^-7 nm

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24
Q

Which light of visible spectrum have shortest wavelength?

A

Purple (4 x 10^-7nm)

Shortest wavelength,highest frequency and highest energy

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25
Which light of visible spectrum have shortest wavelength?
Red (7 x 10^-7nm) Longest wavelength,lowest frequency and lowest energy
26
Which light of visible spectrum have highest energy?
Purple
27
Which light of visible spectrum have highest energy?
Red
28
The electrons closest to the. nucleus is ____ in energy
Lowest
29
Electrons release energy when it_____.
Move from one orbital to another
30
The energy of the electrons released is equal to the energy of _____.
E electron=E photon E=hv
31
Which electron transition involves the greatest release of energy? 1. n=2 to n=6 2. N=6 to n=4 3. N=1 to n=7 4. N= 3 to n=1 5. N=7 to n=2
Ans=4 (bcus n=1 Lowest energy level) Energy given out is maximum when the electron from the higher state falls into the lowest energy subshell. DO NOT DECIDE BY DIFFERENCE IN NUMBERS
32
What rays is released when electrons fall to n=1 level?
UV rays (Lymen series)
33
What rays is released when electrons fall to n=2 level?
Visible light spectrum (Balmer series)
34
What rays is released when electrons fall to n=3 level?
IR (Paschen serie)
35
What rays is released when electrons fall to n=4 and n=5 level?
IR (Bracket serie)
36
First ionization energy means____
The amount of energy released when one mole of electrons is removed from one mole of gaseous atoms in their ground state.
37
Why do the lines coverage at higher energies?
Bcuz energy levels inside the atom are closer together at the higher energy Eg 3s and 4 d energy levels are similar——-> transition metals have variable oxidation numbers
38
What is absorption spectrum?
The spectrum that shows when electron moves from higher energy level to lower energy level. The absorption spectrum can be seen as blacklines in visible light spectrum.
39
What is emission spectrum?
The spectrum that shows when electron moves from lower energy level to higher energy level. The emission spectrum can be seen as lines in black background. (visible only when hih voltage is applied)
40
Emission light spectrum and absorption light spectrum, which can be used to guess the electronic configuration?
Emission spectrum ——> analyse ——> information about the electronic configuration of different atoms
41
Each orbital can hold only ——- electrons
Two Eg, p orbitals ——-> 6 electrons Px Py Pz - 2 electrons each
42
How many sub orbitals are there in energy level 1 ,2 , 3 and 4?
1 -s 2 - s+ p 3- s+ p+d 4- s+p+d+f S orbital - 1 atomic orbital P orbital - 3 atomic orbital px py pz D orbital - 5 atomic orbital — — — — — F orbital- 7 atomic orbital — — — — — — —
43
Shape of s orbital
Spherical shape
44
Shape of p orbital
Dumbbell shape (arranged at 90 degree to each other)
45
Shape of d orbital
Clover-leaf shape
46
List the 4d,4f,4p and 4s atomic orbitals in increasing energy.
4f-----4d------4p-----4s
47
State the number of 4d,4f,4p and 4s atomic orbitals.
4s-1 4p-3 4d-5 4f-7
48
How to calculate the number of electrons in energy level?
2n²
49
When adding electrons to the orbitals, the electrons are filled first in ——— orbital
Lower energy
50
Electronic configuration of calcium
1s²2s²2p63s²3p6 4s² [Ar] 4s²
51
Unpaired electron present in phosphorus
15P- 1s2 2s2 2p6 3s2 3p3 Unpaired electrons -3
52
How many orbitals are located in the 3 energy level?
9 1s 3p 5d
53
Unpaired electron present in vanadium (Z=23)
1s2 2s2 2p6 3s2 3p6 4s2 3d3 Unpaired electrons=3
54
What are 2 elements that deviate from Pauli rule?
Chromium(Z=24) & copper(Z=29)
55
Electronic configuration of Chromium
1s² 2s² 2p⁶ 3s² 3p⁴ 3d⁵ 4s¹
56
Electronic configuration of copper
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰
57
Electronic configuration of Cr3+
1s2 2s2 2p6 3s2 3p6 3d3
58
Electronic configuration of S2-
1s2 2s2 2p6 3s2 3p6
59
Electronic configuration of Fe3+
1s2 2s2 2p6 3s2 3p6 4s0 3d5
60
Once the ionization energy is added to remove an electron from the atom, the electron is taken away from the nucleus and can be considered to be n= ———
Infinity
61
Mass and charge of proton and electron
Mass- 1 amu or 1.67*10-24g Mass of an electron -0.00055 amu Charge of a proton = + 1.67*10-19 coulomb Charge of an electron= - 1.67*10-19 coulomb
62
The mass of an atom is determined by ———
Mass of a proton and neutron bcuz electron mass is negligible
63
The number of—— is the defining traits of the element 1. Proton 2. Electron . 3 Neutrons
1. Proton bcuz the atomic number——> trait of an electron, no matter how many electrons or neutrons it may have
64
An ion of platinum has a mass number of 195 and contains 74 e, how many protons and neutrons does it contain? What is the charge? Z=78
The number of protons -78 The number of neutrons - 195- 78 = 117 Charge = +4
65
One element that does not have neutron
Hydrogen 1 H 1
66
How can we find the atomic mass of an element ?
Mass number = no of protons + no of neutrons = 1 amu+ 1amu ( approximately)
67
the atomic mass of an element should be equal to the mass number. But there are slight variations, WHY?
Bcuz of the existence of isotopes.
68
Relative atomic mass formula
(Relative abundance of an isotope* mass number + relative abundance of second isotope* mass number of 2nd isotope ) / the number of atoms
69
Valence electrons of transition elements
D subshell - unfulfilled electrons in d subshell + adjacent s subshell electrons Eg valence electrons of Cu- (Ar) 4s13d10 Valence electron =1 In the above case, valence electrons in d subshell are filled therefore, take the electrons number in adjacent s orbital only Valence electrons of vanadium -(Ar) 4s2 3d1 Valence electron =3

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