Electrons in Atoms and Ions Flashcards

1
Q

What is an orbital?

A

a region of space that can hold up to 2 electrons with opposite spins. It has a specific energy level.

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2
Q

How are the shapes of orbitals denoted?

A

s
p
d
f

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3
Q

What is the shape of an s orbital?

A

circle
has a spherical boudary surface

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4
Q

What is the shape of a p orbital?

A

“dumbbell” shaped
infinty shaped

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5
Q

What is a shell?

A

a group of orbitals denoted by the same number (they are mathematically related)

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6
Q

How are orbitals in the same shell similar?

A

they are generally similar in size so the average distance from the nucleus is similar

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7
Q

How are the energy levels in orbitals related?

A

they are similar but not the same

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8
Q

What happens when the number of shells increases?

A

the orbitals within the shell become larger = the average distance from the nucleus of the electrons within the orbitals increases = the energy of the electrons also increases

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9
Q

How are the p orbitals in a shell arranged?

A

at right angles to each other

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10
Q

How many s orbitals in a shell?

A

1

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11
Q

How many p orbitals in a shell?

A

3

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12
Q

How many d orbitals in a shell?

A

5

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13
Q

How many f orbitals in a shell?

A

7

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14
Q

How many electrons are in a s orbital?

A

2

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15
Q

How many electrons are in a p subshell?

A

6

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16
Q

How many electrons are in a d subshell?

17
Q

How many electrons are in a f subshell?

18
Q

How do electrons arrange themselves in an orbital?

A

occupy as many is neccessary, starting with those of the lowest energy
elecrtons will pair up in an orbital
electrons will go in different subshells to start - they do not pair up

19
Q

Why don’t electrons pair up in orbitals initially?

A

it gives a lower overall energy state which reduces the repulsion between electrons

20
Q

What is a sub-shell?

A

groups of orbitals of the same type, they are named according to the shell they are in and the orbital type
eg 2p

21
Q

What is reflected in the periodic table?

A

the relative energies

22
Q

Where are the s block elements?

A

group 1 and 2

23
Q

Where are the p block elements?

A

Group 3,4,5,6,7,0

24
Q

Where are the d block elements?

A

transition metals

25
What happens when a +ion is formed in terms of electrons?
the highest energy electrons are lost first
26
What happens when a -ion is formed in terms of electrons?
extra electrons are added to the highest energy subshell until it is full
27
Why does the 3d subshell come after the 4s subshell when DRAWING the electron configuration?
it has a higher energy than 4s but lower energy than 4p
28
Why does the 3d subshell come before the 4s subshell when WRITING the electron configuration?
4s looses electrons first
29
What classifies elements as p-block (any block) elements?
their electron configuration ends in P
30
What element forms a 1- ion with the same electron configuration as He?
H