Quiz 2

Question 1

Define chemistry

Answer 1

The science of the structure and interactions of matter

Question 2

Define matter

Answer 2

Anything that occupies space and has a mass

Question 3

Define mass

Answer 3

The amount of matter a substance has

Question 4

Define weight in relation to mass

Answer 4

Weight is the force of gravity acting on a mass

Question 5

Define chemical elements

Answer 5

Building blocks of all matter living and nonliving

Question 6

Define atoms

Answer 6

Smallest unit of matter that retains the properties and characteristics of that element

Question 7

Atomic number

Answer 7

Number of protons in an element

Question 8

Mass number

Answer 8

Sum of protons and neutrons in an element

Question 9

Define atomic mass/weight

Answer 9

Average mass of all naturally occurring isotopes

Question 10

Define isotopes

Answer 10

Atoms of an element that have different numbers of neutrons and therefore a different mass number

Question 11

Define ion

Answer 11

An atom or molecule that gives up or gains an electron and therefore has a charge

Question 12

Define compounds

Answer 12

Contains atoms of 2 or more different elements

Question 13

Electrolytes

Answer 13

Ionic compound that breaks down into cations and anions in a solution

Question 14

Octet rule

Answer 14

An atom needs 8 electrons in its valence shell to be stable. Atoms are more likely to interact if doing so will leaveboth valence shells with 8 elections

Question 15

What makes noble gases special?

Answer 15

They are stable on their own because they have a full valence shell. They don’t need to bond.

Question 16

Ionic bonds

Answer 16

Cations and anions attract each other due to the opposition of charges. Usually exist in solids. Found mostly in teeth, bones

Question 17

Nonpolar covalent bonds

Answer 17

2 or more atoms share electrons evenly. Can form between atoms of the same or different elements. Can share up to 3 pairs of Valence elections

Question 18

Polar covalent bonds

Answer 18

Electrons shared unevenly due to electronegativity. Nucleus of bigger atom attracts the shared electron more strongly so it becomes partially negative. The smaller electron becomes slightly more positive.

Question 19

Electronegativity

Answer 19

The measure of an atom’s ability to attract shared elections to itself.

Question 20

Hydrogen bonding

Answer 20

Weak bond that occurs due to the polarity of polar covalent bonds- not really a solid bond, more of an attraction.results from attraction of oppositely charged sharing of electrons

Question 21

Free radical

Answer 21

Atom or group of atoms with an unpaired election in the outermost shell. Unstable, highly reactive, destructive to nearby molecules. Antioxidants inactivate them.

Question 22

Radioactivity

Answer 22

When unstable atoms spontaneously break themselves down to reach a stable state. Breakdown causes radioactivity.

Question 23

Half-life

Answer 23

Time it takes for half the atoms of a radioactive substance to break down into a more stable form.

Question 24

Law of conservation of mass

Answer 24

Mass cannot be created or destroyed

Question 25

Law of conservation of energy

Answer 25

Energy cannot be created or destroyed) only transferred

Question 26

Potential energy

Answer 26

Energy stored by matter due to position (think holding up a ball)• static, waiting to be used.

Question 27

Kinetic energy

Answer 27

Associated with matter in motion (think after you let go of the ball and it falls to the ground)

Question 28

Exergonic reactions

Answer 28

Reactants start with energy and products have less energy after reaction (catabolic). Extra energy is released.

Question 29

Endergonic reactions

Answer 29

Reactants start without energy and products gain energy (anabolic). Energy is required for the reaction. Absorb more energy than is released.

Question 30

Metabolism

Answer 30

The sum of all chemical reactions in the body. Coupling of exergonic and endergonic reactions - energy released from exergonic usually used to drive endergonic.

Question 31

Activation energy

Answer 31

Energy required for a reaction to occur. Reactions depend on concentration and temperature. High concentration of atoms means there are more atoms available to bond. High temperature makes atoms more around a lot, increasing likelihood of forming bonds.

Question 32

Catalysts

Answer 32

Help speed up reactions by lowering amount of activation energy needed to start a reaction. Ex. Enzymes in the body.

Question 33

Synthesis

Answer 33

Chemical reaction where the resulting product is bigger than the reactants. Bonds formed. Anabolism. Usually endergonic.

Question 34

Decomposition

Answer 34

Chemical reaction where resulting products are smaller than reactants. Bonds broken. Aka catabolism. Usually exergonic.

Question 35

Exchange reactions

Answer 35

Ab+cd = ad + BC

Question 36

Reversible reactions

Answer 36

Ab ←→ a+b

Question 37

Inorganic vs. Organic compounds

Answer 37

Inorganic usually doesn't contain carbon. Organic always has carbon, usually hydrogen and always covalent bonds. Organic compounds are more complex.

Question 38

H2O has polarity. T/f

Answer 38

True

Question 39

Hydrolysis

Answer 39

Breakdown of large molecules into simpler ones with H2O

Question 40

Dehydration synthesis

Answer 40

2 simple molecules join together, eliminating H2O in the process.

Question 41

Dehydration synthesis vs. Hydrolysis

Answer 41

H20 is the product in dehydration synthesis, but the reactant in hydrolysis

Question 42

Ionization

Answer 42

The process by which ions are formed by gain or loss of an electron from an atom or molecule.

Question 43

Hydrophilic

Answer 43

Dissolves in H20. Has polar covalent bonds.

Question 44

Hydrophobic

Answer 44

Not water soluble

Question 45

Mixture

Answer 45

Combo of elements or compounds physically blended together but not bound by chemical bonds.

Question 46

Solutions

Answer 46

Solutes mixed into a solvent are evenly distributed (transparent)

Question 47

Colloids

Answer 47

Size of particles of solvent larger than in a solution so it is opaque. Ex. Milk

Question 48

Suspension

Answer 48

Suspended material may mix at the beginning but will settle out. Ex. Muddy water.

Question 49

Concentration

Answer 49

How much solute is found in the solvent. Moles per litre (moL/L) = morality

Question 50

Acid

Answer 50

Proton donor, pH below 7

Question 51

Base

Answer 51

Proton acceptor. pH above 7

Question 52

Salt

Answer 52

Electrolytes- acids and bases react to form salts.

Question 53

Buffer systems

Answer 53

Used to convert strong acids and bases into weaker ones. they remove or add protons.

Question 54

Carbohydrates

Answer 54

Function mainly as a source of chemical energy for generating ATP. Formed via carbon, hydrogen, oxygen. 2:1 H:O. 1 H2O per C. sugars, glycogen, starches, cellulose

Question 55

3 major groups of carbs

Answer 55

Monosaccharides, disaccharides, polysaccharides

Question 56

what are simple sugars made up of

Answer 56

monosaccharides and disaccharides (combo of 2 monosaccharides through dehydration synthesis). end in -ose.

Question 57

characteristics of simple sugars

Answer 57

can be absorbed without need to digest further. use hydrolysis to break down disaccharides and polysaccharides

Question 58

how are saccharides joined together

Answer 58

dehydration synthesis

Question 59

polysaccharides

Answer 59

- many monosaccharides joined together through dehydration synthesis - glycogen is the main one found in the body. - hydrolysis can break them down into monosaccharides. - found in starches

Question 60

where in the body is glycogen stored

Answer 60

liver and skeletal muscle

Question 61

what is the storage form of glucose in the body

Answer 61

glycogen