3- exceptions for electron configurations Flashcards

1
Q

Anion rules

A

Anion Rules
Add the extra electrons corresponding to the ion charge to the total number of electrons in the neutral atom before proceeding to write the configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Cation Rules

A

Cation Rules
Write the configuration for the neutral atom first
Remove the electrons from the orbital from the highest period number, n, as these represent the electrons in the valence shell

remove electrons from the highest period number (as these electrons are the furthest away)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Explaining Charges

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Recognizing atoms in their excited states

A

Excited state –> electrons have gained energy and moved into a higher orbital, the total number of electrons in the atom have not changed
Count the number of electrons to determine the atom

The electron configurations below represent atoms in their excited states. Identify each atom and write its ground state electron configuration.

compare ground state (normal configuration) to excited state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Exceptions for writing electron configurations d-orbitals

A

Half filled and fully filled d-orbitals are more stable
know these exceptions!

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Key Ideas of Lewis theory of bonding are:

A

Atoms and ions are stable if they have a noble gas like electron structure i.e., a stable octet of electrons
Electrons are most stable when they are paired

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

how can we achieve a stable octect?

A

Atoms form chemical bonds to achieve a stable octet of electrons in two (2) ways:
1) exchanging electrons between metal and non-metal atoms (ionic bonding) OR
2) sharing electrons between non-metal atoms (covalent bonding)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

rules for drawing lewis dot diagrams –> Which atoms go to the middle and which atoms surround the central atom?

A

Rule 1: The central atom is usually the least electronegative atom
Rule 2: Other atoms surround the least electronegative atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What must you do after placing the atoms in your diagram?

A

Rule 3: Count the total number of valence electrons, including charges
-1 ionic charge = gained 1 electron = +1 electron
+2 ionic charge = lost 2 electrons = -2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

how to distribute electrons after counting for our diagram?

A

Rule 4: Place electron pairs between each atom to represent a single bond, then distribute the remainder of the electrons around the surrounding atoms to satisfy octet rule. [Any remaining electrons that have not been distributed can be placed on the central atom as lone pairs]

[Should an octet not be satisfied on central atom, non-bonding electrons on the outer atoms can be used to create a double bond]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How to finish a lewis dot diagram drawing?

A

Rule 5: Replace electrons with lines to represent bonds and place square brackets around the final structure. Indicate the charge on the structure by placing the charge on the outside of the right square bracket.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

resonance structures

A

When more than one Lewis structure can be drawn, the molecule or ion is said to have resonance / resonance structures (ie. the double/triple bond can move in the complex)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Formal Charge (FC)

A

V = total number of valence electrons
N = number of non-bonding electrons
B = number of bonds
Single bond = 1
Double bond = 2
Triple bond = 3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

why do we use formal charge?

A

A molecule will not allow for both positive and negative formal charges to exist within its structure. To adjust, electron pairs are moved from the negative atoms to form bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly