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chemistry > electron structure > Flashcards

electron structure Flashcards

1
Q

What is the shape of an s-orbital

A

speherical

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2
Q

How many electrons can be held in a d-subshell

A

10

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3
Q

How many electrons can fill the f-subshell

A

14

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4
Q

How many electrons can an orbital hold

A

2

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5
Q

How many electrons can the 4th shell hold?

A

32

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6
Q

How many electrons can be held in a p-subshell

A

6

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7
Q

how many orbitals are found in a s-subshell

A

1

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8
Q

What is a shell

A

A group of orbitals with the same principle quantum number

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9
Q

What is the equation for how many electrons each subshell holds

A

2n2

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10
Q

How many electrons can the 1st shell hold?

A

2

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11
Q

Why does the 4s orbital fill before the 3d orbital

A

4s orbital has a lower energy than 3d before it is filled

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12
Q

What are the rules by which electrons are arranged in the shell?

A
  1. Electrons are added one at a time
  2. Lowest available energy is filled first
  3. Each energy level must be filled before the next one can fill
  4. Each orbital is filled singly before pairing
  5. 4s is filled before 3d
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13
Q

How many orbitals does a p-subshell have

A

3

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14
Q

How many orbitals are present in a D-subshell

A

5

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15
Q

How many orbitals are found in an F-subshell

A

7

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16
Q

Which electrons are lost when atom becomes a positive ion

A

Electrons in the highest energy levels

17
Q

How many electrons can the 2nd shell hold?

A

8

18
Q

what is the shape of a p-orbital

A

dumb-bell shape

19
Q

What does the principal quantum number (1s2 2s2 etc..) indicate?

A

The shell occupied by the electrons

20
Q

How many electrons can be held in an s-subshell

A

2

21
Q

How many electrons can the 3rd shell hold?

A

18

22
Q

What are the 4 types of orbitals

A

s-orbital
p-orbital
d-orbital
f-orbital

23
Q

Define an orbital

A

A region around the nucleus that can hold up to two electrons with opposite spins

chemistry (37 decks)

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