Chemistry > Electronic configuration > Flashcards

Electronic configuration Flashcards

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1
Q

2nd energy

A

Contains one 2s and three 2p orbitals
can hold 10e

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2
Q

A region where electrons are likely to found in space is called

A

Orbits

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3
Q

Angular momentum quantum number(l) describe

A

shape of the subshell

l=0 to (n-1)

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4
Q

As the orbital becomes far from nucleus,which energy increases and which decreases?

A

The energy of the orbitals and energy of the electron increases and the energy of nuclear attraction decreases

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5
Q

Atoms that deviate the Aufbau principle

A

Cr(Z=24) & Cu(Z=29)

*Half-filled & fully-filles d subshells are more stable.

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6
Q

Atoms with the unpaired electrons are

A

Paramagnetic (affected by magentic field)

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7
Q

Atoms without the unpaired electrons are

A

Diamagnetic (not affected by magentic field)

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8
Q

Aufbau Principle

A

Electrons must be filled in the orbitals from lowest to highest energy level

1s,2s,2p,3s,sp,4s,3d,4p,….

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9
Q

Each electron shell is divided into ______.

A

Different subshells (s,p,d,f)

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10
Q

Each orbital can hold only ——- electrons

A

Two
Eg, p orbitals ——-> 6 electrons Px Py Pz - 2 electrons each

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11
Q

Electronic configuration of calcium

A

1s²2s²2p63s²3p6 4s²
[Ar] 4s²

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12
Q

electronic configuration of calcium

A

20Ca-1s2 2s2 2p6 3s2 3p6 4s2

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13
Q

Electronic configuration of Chromium

A

1s² 2s² 2p⁶ 3s² 3p⁴ 3d⁵ 4s¹

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14
Q

Electronic configuration of copper

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰

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15
Q

electronic configuration of Cr3+

A

24 Cr 3+____1s2 2s2 2p6 3s2 3p6 4s2 3d3

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16
Q

Electronic configuration of Cr3+

A

1s2 2s2 2p6 3s2 3p6 3d3

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17
Q

Electronic configuration of Fe3+

A

1s2 2s2 2p6 3s2 3p6 4s0 3d5

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18
Q

electronic configuration of S2-

A

16S2-____1s2 2s2 2p6 3s2 3p6

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19
Q

Electronic configuration of S2-

A

1s2 2s2 2p6 3s2 3p6

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20
Q

Electrons are arragned in _______ in the atom.

A

Shells or energy levels (K,L,M,N)

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21
Q

Electrons in same subshells are in same energy.True or False?

A

True

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22
Q

Elements whose valence electrons in d sub level make up_____ of periodic table

A

d block

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23
Q

Elements whose valence electrons in f sub level make up_____ of periodic table

A

f block

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24
Q

Elements whose valence electrons in p sub level make up_____ of periodic table

A

p block

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25
Elements whose valence electrons in s sub level make up_____ of periodic table
s block
26
Energy levels of shell are ______.
different
27
Energy shell farest to the nucleus have the _____ energy level.
Highest
28
Energy shell nearest to the nucleus have the _____ energy level.
Lowest
29
Every electrons have their own unique quantum numbers.True or False?
True No 2 electrons have same quantum number
30
First energy level
contains one 1s orbital Lowest energy level Can hold 2e
31
How do you find the valence electrons in atoms?
By looking at the electronic configuration,electrons in the highest energy shell is the valence electrons
32
How electrons are arranged in first 3 shells?
The 1st shell can hold only 2e and it fills first. The 2nd shell can hold 8e and it fills second. The 3rd shell can hold 18e but it fills up to 8 and the next 2 go to 4th shell finally the rest are filled to 3rd shell. 288
33
How many orbitals are located in 3rd energy level?
1s+3p+5d=9
34
How many orbitals are located in the 3 energy level?
9 1s 3p 5d
35
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 — — — — — — —
36
How to calculate the number of electrons in energy level?
2n²
37
Hund's Principle
Electrons must fill in orbitals singly before start pairing up. *to reduce electron replusion
38
Hund’s rule
If more than one orbital in a sub-level is available,electrons occupy different orbitals with parallel spins
39
l=0,the electron is in______.
s subshell
40
l=1,the electron is in______.
p subshell
41
l=2,the electron is in______.
d subshell
42
l=3,the electron is in______.
f subshell
43
List the 4d,4f,4p and 4s atomic orbitals in increasing energy.
4f-----4d------4p-----4s
44
Magnetic Quantum Number (ml) describe
orbital orientiation ml=-1 to +1
45
Maximum number of electrons in each shell
2n^2
46
Number of orbit in d subshell
5 orbital
47
Number of orbit in f subshell
7 orbitals
48
Number of orbit in p subshell
3 orbital (x,y,z)
49
Number of orbit in s subshell
only 1 orbital
50
number of sub orbitals in each orbital
s-1 p-3 d-5 f-7
51
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
52
Orbits in the same subshell only differ in _______.
Orientation
53
Pauli Exclusion
No more than two electrons can occupy any one orbital, and if 2e are in same orbital they must spin in opposite directions
54
Pauli Exclusion Principle
No 2 electrons can have same set of 4 quantum numbers.If n,l,ml are same, ms can be different. Electrons in each orbitals spin in opposite direction(Spin-pairing)
55
Prinicipal quantum number(n) describe
the energy level of electron n=1,2,3,4,.....
56
Quantum number of electrons
principal quantum number (n) azimuthal quantum number (l) magnetic quantum number (ml) spin quantum number (ms)
57
Quantum Numbers
Specific number set that can determine the position of electron in an atom
58
Shape of d orbital
Clover-leaf shape
59
shape of d subshell
Clover leaf shaped
60
Shape of f subshell
Complex shape
61
Shape of p orbital
Dumbbell shape (arranged at 90 degree to each other)
62
Shape of p subshell
Dumbbell shape
63
Shape of s orbital
Spherical shape
64
Shape of s subshell
Spherical shape
65
Spin Quantum Number (ms) describe
how the electron spin Ms=+1/2 or -1/2
66
State the number of 4d,4f,4p and 4s atomic orbitals.
4s-1 4p-3 4d-5 4f-7
67
The energy of the 1st shell
Since it is the closest to the nucleus and it has lowest energy level
68
the formula of number of electrons in the energy level
2n^2 (squared)
69
Unpaired electron present in phosphorus
15P- 1s2 2s2 2p6 3s2 3p3 Unpaired electrons -3
70
Unpaired electron present in vanadium (Z=23)
1s2 2s2 2p6 3s2 3p6 4s2 3d3 Unpaired electrons=3
71
What are 2 elements that deviate from Pauli rule?
Chromium(Z=24) & copper(Z=29)
72
What are the differences between main group elements and transition elements?
Main group elements have outermost electrons added to s and p sub-shell.if the electrons are in d sub-shell,they are fully filled(10e in d sub-shells)
73
What is an atomic orbital?
a region around nucleus in which there is 90% probability of finding the electrons
74
What is electron shell?
Electrons are arranged in shells around nucleus.
75
What is the electronic configuration of Cr 24?
1s2 2s2 2p6 3s2 3p6 4s1 3d5 (d sub shellမှာhalf filled ဖြစ်ချင်လို့ 4sကနေတစ်လုံးယူ)
76
What is the electronic configuration of Cu 29?
1s2 2s2 2p6 3s2 3p6 4s1 3d10 (d sub shellမှာfully filledဖြစ်ဖို့4s sub shellကနေone electronယူ)
77
What is the valence electrons of gallium? Ga=31
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 (3d=10eမလို့ 4s and 4pမှာvalence electron=3)
78
What is transition elements?
Partially filled electrons in d-sub shells But Cu,Zn,Au,Ag, Hg have fully filled electrons in d sub shell, but they are transition elements group in periodic table
79
When adding electrons to the orbitals, the electrons are filled first in ——— orbital
Lower energy
80
Which orbital has lowest energy level?
The orbital closest to the nucleus has the lowest energy n=1
81
_______ in the orbital diagram responsible for compound formation.
Unpaired or valence electrons
82
How transition metals lose electrons?
They lose electrons from 4s sub level before 3d sub level
Chemistry
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