2.3 Electron Configurations Flashcards Preview

Chemistry Chapter 2 - Atomic Structure > 2.3 Electron Configurations > Flashcards

Flashcards in 2.3 Electron Configurations Deck (21):
1

How are electrons arranged in an atom?

Energy levels round nucleus.

2

How are the maximum number of electrons in each main energy level found?

2n^2 where n is the number of main energy level.

3

What are the main energy levels divided up into?

Sub shells - s, p, d, f

4

What are the maximum number of electrons in each sub shell?

s - 2
p - 6
d - 10
f - 14

5

Within any main ever level what is the ordering of the sub levels?

s < p < d < f

6

Which sub level is lower in energy than the 3d sub level.

4s

7

What are condensed electron configurations?

Electron configuration of previous noble gas is assumed and everything after that is given in full.

8

What are the two exceptions in electron configuration?

Copper and Chromium - instead of having normal electron configurations they only have one electron in the 4s sub level.

9

What is the electron configuration of copper?

Cu: 1s2 2s2 2p6 3s2 3p6 3d5 4s1

10

What is the electron configuration of chromium?

Cr: 1s2 2s2 2p6 3s2 3p6 3d10 4s1

11

What is an orbital?

A region of space where there is a high probability of finding an electron.

12

What energy does an orbital represent?

Each orbital represents a discrete energy level.

13

How many electrons can an orbital contain?

A maximum of two electrons with opposite spins.

14

What are the shapes of s and p orbitals?

s is spherical
p is dumbbell shape

15

How are the p orbitals arranged?

px points along x axis
py points along y axis
pz points along z axis

16

What is each sub level made up of?

A set of degenerate orbitals.

17

What does an orbital diagram show?

Electrons as single headed arrows in boxes, each box represent an orbital. Arrows point either up or down representing electrons spinning in opposite directions.

18

What is the Pauli exclusion principle?

Maximum number of electrons in an orbital is two - if there are two electrons in an orbital they have opposite spin..

19

What is Hund's rule?

Electron fill orbitals of same energy as to give the maximum number of elections with spins the same.

20

What happens for electron configuration of positive ions?

Highest energy electrons are removed first.

21

What happens for the electron configuration of positive ions for transition metals and elements in group 13 and 14?

4s electrons and removed before 3d electrons.