Module 1

Question 1

Define Chemistry

Answer 1

Study of matter and the changes it undergoes

Question 2

Organic chemists

Answer 2

Study carbon-based compounds; there are more carbon compounds than non-carbon compounds.

Question 3

Biochemistry

Answer 3

Study chemical processes within living systems; application of chemical processes to living systems

Question 4

Physical chemists

Answer 4

Glorified mathemeticians

Question 5

Define Matter

Answer 5

Anything that has mass and occupies space

Question 6

Atoms

Answer 6

Submicroscopic particles that are building blocks of all matter

Question 7

Protons

Answer 7

Positively charged particle with sizable mass; Determines the identity of an atom, extremely difficult to change

Question 8

Neutrons

Answer 8

Electrically neutral, mass equivalent to proton. This tells us what isotope we are dealing with

Question 9

Electrons

Answer 9

Negatively charged particles with a very small mass; tells us the charge of the atom, easy to change. Metals like to lose electrons.

Question 10

Molecules

Answer 10

Two or more atoms in a specific arrangement

Question 11

Solids

Answer 11

Densely packed molecules, definite shape, not very compressible.

Question 12

Liquid

Answer 12

Loosely packed molecules, no definite shape, not easily compressible.

Question 13

Gas

Answer 13

Molecules are not packed, no shape, easily compressible.

Question 14

What happens if gas compresses too much?

Answer 14

Liquifies

Question 15

What does it mean if a gas tank is empty?

Answer 15

Means the pressure inside the tank is equal to the pressure of the atmosphere outside the tank.

Question 16

Pure substance

Answer 16

Single type of matter, only one type of molecule.

Question 17

Element

Answer 17

Only one type of atom, cannot be broken into separate atoms (e.g. iron metal is only FE)

Question 18

Compound

Answer 18

One type of molecule but can be broken into separate atoms. (e.g. H2O)

Question 19

Mixture

Answer 19

2 or more pure substances that retain their own identities and can be broken

Question 20

Homogenous mixture

Answer 20

Looks the same throughout, uniform composition. (e.g. Apple juice)

Question 21

Heterogenous mixture

Answer 21

Looks different throughout, not uniform in composition (e.g. salad dressing)

Question 22

Physical change in matter

Answer 22

Change that alters state or appearance, but not composition. (e.g. Ice cube is solid, water is liquid, gas is clouds. All of it is H20)

Question 23

Condensation, deposition, sublimation

Answer 23

Gas to liquid, gas to solid, solid to gas

Question 24

Chemical changes in matter

Answer 24

Change that alters COMPOSITION (e.g. iron rusting and going from FE to Fe2O3)

Question 25

Physical change vs chemical change examples

Answer 25

Physical: cutting firewood
Chemical: burning firewood

Question 26

Physical properties of matter

Answer 26

Property displayed by a substance that doesn’t change in its composition (e.g. Odor, taste, color, appearance, melting/boiling point)

Question 27

Chemical properties of matter

Answer 27

Property displayed by a substance caused by CHANGE IN COMPOSITION (e.g. Corrosiveness, flammability, acidity, toxicity)

Question 28

Atomic theory overview

Answer 28

Tiny, indestructible atoms. All atoms of a given element have same mass, atoms combine to form compounds, atoms can change the way they bind to other elements but cannot change the atoms of that element.

Question 29

Protons and neutrons are bound together by ______ forces into an incredibly dense structure called the ________.

Answer 29

Nuclear, nucleus.

Question 30

Electrons are bound to the nucleus by ______.

Answer 30

Electromagnetic forces.

Question 31

Name of group 1 on the period table

Answer 31

Alkaline metals

Question 32

Name of group 2 on the period table

Answer 32

Alkaline earth metals

Question 33

Name of group 17 on the period table

Answer 33

Halogens

Question 34

Name of group 18 on the period table

Answer 34

Noble gases

Question 35

Groups 3-12 on the periodic table are called

Answer 35

Transition elements

Question 36

Atomic number

Answer 36

Number of protons in an element

Question 37

Groups 13-18 on the period table, how do you figure the amount of valence electrons they have?

Answer 37

Subtract 10 from the group number

Question 38

Carbon has an atomic number of 6, in group 14. How many total electrons does it have?

Answer 38

2 core, 4 valence.

14-10 is 4 (valence), and the atomic number is 6. So it must have 2 core.

Question 39

Shape of S atomic orbital

Answer 39

Sphere

Question 40

Shape of P atomic orbital

Answer 40

Figure 8

Question 41

Shape of D atomic orbital

Answer 41

Clover leaf

Question 42

Core electrons. Where are they and are they involved in chemical bonding?

Answer 42

Inner most electrons that occupy lowest energy levels. They are not involved in chemical bonding!

Question 43

Valence electrons: where are they and are they involved in chemical bonding?

Answer 43

Outermost that occupy the highest energy levels. They are involved in chemical bonding.

Question 44

Aufbau principle

Answer 44

Electrons are placed into orbitals of the lowest available energy

Question 45

Atomic size by group and period?

Answer 45

Increases as you move down (groups) and to the left (period)

Question 46

Ionic size (size of anions vs cations)

Answer 46

Cations are smaller than anions

Question 47

Electronegativity

Answer 47

Ability to attract electrons. Decreases as you move down in the group, and to the left of the period.