Bonding and Structure

Question 1

T/F: Atoms form bonds to raise their potential

Answer 1

FALSE, they form bonds to lower their potential

they want lower energy= more stable

Question 2

Octet rule

Answer 2

Main group elements bond in such a way that each atom has eight electrons (a completed valence)

Question 3

What types of bonds are there?

Answer 3

Ionic and Molecular

Question 4

Ionic Bonding is?

Answer 4

Electrons are transferred from one entity to another

Stronger than covalent

(electrostatic interaction; charges attract each other)

Question 5

What properties effect ionic bonding?

Answer 5

Ionization energy: able to give up electron with low energy

Electron affinity: likelihood of an atom to pick up an additional electron density (trying to add more to it)

Question 6

Difference between electronegativity and electron affinity.

Answer 6

Electronegativity: how well it holds the electrons within it

Electron affinity: likelihood of an atom to pick up an additional electron density (trying to add more to it)

Question 7

T/F: Metals want to give up electrons; nonmetals want to gain electrons

Answer 7

TRUE

Question 8

Explain covalent bonding

Answer 8

Electrons are SHARED between atoms

Forms bonds.

Question 9

Polar Covalent Bond

Answer 9

Electrons are NOT EQUALLY shared with the electron density residing towards the more electronegative atom

Question 10

Nonpolar Covalent Bond

Answer 10

Electrons are essentially shared equally between the atoms

Question 11

How to denote that one atom has a greater share of the electrons.

Answer 11

Question 12

T/F: Lewis Structures represent the VALENCE electrons and the bonds

Answer 12

TRUE

Question 13

How do you find the valence electrons of elements in the periodic table?

Answer 13

Look at Group #
Only have 1-12 valence electrons–Groups 1=1, etc

Groups 13-18:
Group# - 10 = # of valence electrons

Question 14

Which elements are exceptions to the octet rule?

Answer 14

Hydrogen (two electrons)
Boron (6 electrons)
Aluminum (6 electrons)

Question 15

Expanded Octets occur in what periods?

Answer 15

Period 3 and higher

Question 16

What are expanded octets?

Answer 16

Allows ten or twelve electrons

Occurs due to d-orbitas

Question 17

Steps to drawing molecular compound lewis dot structure

Answer 17

-Count the total number of electrons available

-Draw skeletal structure (central atom + peripheral atoms + bonds)

-Fill octets of peripheral atoms by adding lone pair electrons

-Add any remaining electrons to the central atom as lone pair electrons

-Calculate any formal charges

-Adjust structure to minimize formal charges

Question 18

How to balance our FC charges?

Answer 18

• Move one lone pair from the peripheral atom into a bond with the central atom (single bond -> double bond)

-Move the charge on the peripheral atom one step in the positive direction (-1 -> 0)

-Move the charge on the central atom one step in the negative directions (+1 -> 0)

-Repeat until there no charges on both the central atom and peripheral atom or until you only have one charge on either atom

Question 19

How do you determine the central atom in a Lewis dot structure?

Answer 19

Whichever atom has the lowest electronegativity; or usually least amount atom

Question 20

How many bonds can hydrogen form?

Answer 20

One

Question 21

AX2

Answer 21

Linear (180)

Question 22

AX3

Answer 22

trigonal planar (120)

Question 23

AX2E

Answer 23

Bent (<120)

Question 24

AX4

Answer 24

Tetrahedral (109.5)

Question 25

AX3E

Answer 25

Trigonal Pyramidal (<109.5)

Question 26

AX2E2

Answer 26

Bent (<109.5)

Question 27

AX5

Answer 27

Trigonal Bipyramidal 180,120,90

Question 28

AX4E

Answer 28

See-Saw 180,90

Question 29

AX3E2

Answer 29

T-shaped 180, 90

Question 30

AX2E3

Answer 30

Linear 180

Question 31

AX6

Answer 31

Octahedral 180, 90

Question 32

AX5E

Answer 32

Square Pyramidal 180, 90

Question 33

AX4E2

Answer 33

Square Planar 180,90

Question 34

AX3E3

Answer 34

T-Shaped (180,90)

Question 35

AX2E4

Answer 35

Linear (180)