Chapter 3 Chem 20

Question 1

What are the diatomic molecules that occur naturally

Answer 1

(H) (N) (O) (F) (Cl) (I) (Br) (P) which is 4 and (S) which is 8

Question 2

What is bonding capacity?

Answer 2

Binding Capacity is the atoms availability to bond. EX C has 4 bonding electrons therefore it has a bonding capacity of 4

Question 3

What is the Empirical Formula?

Answer 3

It shows the simplest whole number ratio of the compound.
Rarely used for molecular compounds
EX CH20

Question 4

What is Molecular Formula?

Answer 4

Shows the actual number of atoms that are covalently bonded to make up EACH molecule
Often has elements written in a sequence that helps to determine which atoms are bonded to which
EX C2H4O2 or CH3COOH

Question 5

What is the Lewis Formula?

Answer 5

Often called the Lewis Dot Diagram
it uses Lewis symbols to show electron sharing in covalent bonds
Also shows the formation of stable valence octets of electrons in molecules and ions

Question 6

What is the Structural Formula?

Answer 6

Also commonly called a structural diagram

Instead of using dots, it uses lines to demonstrate the covalent bonds

Question 7

What is the Stereochemical formula?

Answer 7

Similar to structural formula but uses different lines to represent a 3D form
Often not used for bigger compounds because it becomes too complex

Question 8

What is the General Formula?

Answer 8

A formula that indicates how many central atoms, bond pairs, and lone pairs there are

Question 9

What does A mean?

Answer 9

central atom

Question 10

What does X mean?

Answer 10

bond pair

Question 11

What does E mean?

Answer 11

lone pair

Question 12

What is the general formula for linear (2 bond)

Answer 12

AX2 ( 1 central atom, 2 bond pairs)

Question 13

What is the GF for tetrahedral

Answer 13

AX4 (1 central atom, 4 bond pairs)

Question 14

What is the GF for trigonal pyramid

Answer 14

AX3E2 (1 central atoms, 3 bond pairs, and one lone pair)

Question 15

What is the GF for angular

Answer 15

AX2E3 (1 central atom, 2 bond pairs, and 3 lone pairs)

Question 16

What is the GF for trigonal planar

Answer 16

AX3 (1 central atom, 3 bond pairs)

Question 17

What is the GF for angular

Answer 17

AX2E2 (1 central atom, 2 bond pairs, and 2 lone pairs)

Question 18

What is the GF for Linear (1 bond)

Answer 18

AXE3 (1 central atoms, 1 bond pair, and 3 lone pairs)

Question 19

What is the VSEPR theory

Answer 19

A theory based on the electrical repulsion and attraction of bonded or unbonded electrons

Question 20

What are the bases of VSEPR

Answer 20

Valence Shell Electron Pair repulsion

Question 21

What is determined by the position of the electron pairs

Answer 21

The molecular shape

Question 22

What are the types of alignment

Answer 22

Linear 2 (AX2), angular (AX3),  tetrahedrial (AX4),  trigonal Pyramid (AX3E),  Angular (AX2E2),  Trigonal Planar (AX3), 
Linear 1 (AXE3)

Question 23

What are the steps to predicting the shape of a molecule

Answer 23

Step 1 Draw the Lewis Formula and electron pairs
Step 2 Count the total number of bonding pairs and lone pairs around central atom
Step 3 refer to table 7 and use the number of pairs of electrons to predict the shape of the molecule

Question 24

Are bonds stronger or weaker if they are single

Answer 24

weaker

Question 25

Are bonds stronger or weaker if they are double or triple

Answer 25

stronger

Question 26

What is a polar molecule

Answer 26

A molecule where electron charge is not evenly distributed

Question 27

what is a non-polar molecule

Answer 27

A molecule where electron charge (or charge in general) is evenly distributed

Question 28

When is it for sure polar

Answer 28

Diatomic with other atoms (HCl) Containing (N) Containing (O) Containing C with 2 other kind of atoms

Question 29

When is it for sure NOT polar

Answer 29

All elements on their own | Containing (C) and only 1 other kind of atoms

Question 30

What is a polar BOND

Answer 30

Bond that has the different electronegativity

Question 31

What is a non-polar BOND

Answer 31

Bond that has same electronegativity

Question 32

What is a bond Dipole?

Answer 32

When the electrons migrate to one end of the electron creating a difference in charge

Question 33

What are the steps to find polarity

Answer 33

Step 1: draw a Lewis formula Step 2: Use the number of electron pairs and VESPR rules to determine the shape around each central atoms Step 3: Use electronegativities to determine the polarity of each bond Step 4: add the bond dipole vectors to determine whether the result is zero or non-zero

Question 34

When are polar molecules soluble

Answer 34

in other polar substances

Question 35

when are nonpolar substances soluble

Answer 35

in other nonpolar substances

Question 36

what is a intermolecular force

Answer 36

A force within a molecule to attract other molecules to form a shape

Question 37

what is the dipole-dipole force?

Answer 37

An attraction between polar molecules

Question 38

what is the london force?

Answer 38

Momentary attractions between molecules even if they aren't polar

Question 39

How is the strength of the dipole dipole force measured

Answer 39

its measured by the polarity

Question 40

How is the strength of the london force measured

Answer 40

it is measured by the amount of electrons in the molecule and the distance between the molecules

Question 41

What does the bioling point measure

Answer 41

It measures the strength of the bond or intermolecular force

Question 42

What is a isometric molecule?

Answer 42

An isometric molecule is the molecule with the same electron numbers and similar shape

Question 43

What is cohesion

Answer 43

cohesion is an attraction between molecules

Question 44

what is adhesion

Answer 44

adhesion is attraction between opposite molecules

Question 45

what is volatility

Answer 45

volatility is the ability to evaporate

Question 46

what is something the all molecules have in common

Answer 46

they all attract each other through the london force

Question 47

what does fracture mean

Answer 47

fracture is the way solids break