ATOMIC ORBITALS, E CONFIGURATION AND P. TABLE Flashcards

1
Q

How many e can orbitals hold

A

2

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2
Q

What does quantum number n tell us

A

main energy level

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3
Q

What does quantum number l tell us

A

shape of subshell
(values from 0 to n-1)

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4
Q

What does magnetic quantum number m say

A

orientation of orbital
(-l to +l)

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5
Q

What does quantum number s tell us

A

spin

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6
Q

What is the aufbau principle

A

electrons fill orbitals in order of increasing energy

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7
Q

Define Hund’s rule

A

when degenerate orbitals are available, electrons fill each singly,
keeping their spins parallel before spin pairing starts

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8
Q

What is the Pauli Exclusion principle

A

opposite spins

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9
Q

What does it mean if orbitals are degenerate

A

same energy

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10
Q

What do stable electron configurations suggest

A

higher ionisation energy

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11
Q

How many electron pairs does a LINEAR structure have

A

2

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12
Q

How many electron pairs does a TRIGONAL PLANAR structure have

A

3

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13
Q

How many electron pairs does a TETRAHEDRAL structure have

A

4

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14
Q

How many electron pairs does a TRIGONAL BIPYRAMIDAL structure have

A

5

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15
Q

How many electron pairs does a OCTAHEDRAL structure have

A

6

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16
Q

What order does electron repulsion strength decrease in

A

non/non bonding
non/bonding
bonding/bonding