Inorganic Chemistry

Question 1

3 types of mixtures

Answer 1

Suspension, Colloid, Solution

Question 2

Suspension

Answer 2

liquid mixed with solid; cloudy in appearance bc solid particles are visible; will separate/settle if left alone; ex: blood (blood cells suspended in plasma)

Question 3

Colloid

Answer 3

2 distinct components; appears opaque but solid particles are small and not visible to the naked eye; cannot separate/settle; example: milk (proteins are too small to settle but large enough to remain separate)

Question 4

Solution

Answer 4

solid, liquid, or gas mixed with liquid (H2O); translucent due to one substance (solute) dissolving into another (solvent); solubility = degree to which solute gets dissolved; amount of solute = concentration; neither solute nor solvent changes chemically (do not react)

Question 5

Ionic Bonds

Answer 5

bonding that involves the transfer of electrons from one atom to another to satisfy the octet rule (reach 8 valence electrons); when # of electrons change the atom is no longer neutral, resulting in the formation of an ion (+/-); in these bonds, the atoms are held together due to the attraction between the positively and negatively charged ions

Question 6

cations

Answer 6

postively charged ions

Question 7

anions

Answer 7

negatively charges ions

Question 8

covalent bonds

Answer 8

bonding that involves the sharing of electrons to satisfy the octet rule between 2 nonmetals; the strongest chemical bond; can share 1 pair (single bond), 2 pairs (double bond), or 3 pairs (triple bond) of electrons; dont always share the electrons equally

Question 9

nonpolar covalent bond

Answer 9

electrons are shared equally because protons attract electrons equally (electronegativity = how much the protons attract electrons; increases up and across); these bonds have a similar electronegativity/attraction to electrons so neither pulls more than the other and the electrons are shared equally. (1) same element bonded (2) arrangement causes equal pulling (3) bond between carbon and hydrogen

Question 10

polar covalent bonds

Answer 10

electrons are shared unequally due to one atom having a higher attraction to the electrons and pulling them more (high electronegativity difference); causes partial charges on either end creating a dipole (2 poles); still electrically neutral due to equal protons and neutrons

Question 11

hydrogen bonds

Answer 11

bond that forms BETWEEN molecules; the weak attraction between the partially positive hydrogen atoms and partially negative nonmetal atom between 2+ polar covalent molecules; electrons are neither transferred nor shared; responsible for surface tension property of water

Question 12

energy

Answer 12

the capacity to do work (put matter into motion); 2 broad types: kinetic and potential

Question 13

kinetic energy

Answer 13

energy in motion; potential energy can become kinetic when it is used; some sort of work has been done

Question 14

potential energy

Answer 14

energy that is stored; ready to be released to do work; has the potential to do something

Question 15

3 types of potential/kinetic energy

Answer 15

Chemical energy, electrical energy, mechanical energy

Question 16

chemical energy

Answer 16

found in chemical bonds and drives nearly all cellular processes

Question 17

electrical energy

Answer 17

generated by the movement of charged particles; resulted in the body by the flow of ions; allows nerve cells to communicate and plays a role in muscle contractions

Question 18

mechanical energy

Answer 18

energy that is directly transferred between objects;

Question 19

endergonic reaction

Answer 19

reactions that require and input of energy to occur; energy can be thought of as a reactant in the rxn; energy required could be chemical, electrical, or mechanical

Question 20

exergonic reactions

Answer 20

reactants have an excess amount of energy that gets released in the reaction; energy can be thought of as a product; reactant with excess energy considered unstable so it releases energy to become stable

Question 21

Catabolic Reactions

Answer 21

decomposition/ breaking down reaction (large substances broken down to small substances); required to break down nutrients in food, break apart old cells, defend against invaders, etc; generally exergonic due to bonds being broken

Question 22

exchange/redox reactions

Answer 22

1 or more atoms of reactants are exchanged (bonds both broken and formed); oxidation reduction rnxs occur when electrons are exchanged instead of atoms

Question 23

oxidized

Answer 23

reactant in redox rxn that loses electrons (becomes more positve)

Question 24

reduced

Answer 24

reactant in redox rxn that gains electrons (becomes more negative so charge gets smaller/more negative)

Question 25

What affects rate of reaction

Answer 25

concentration, temperature, properties (size/state), and presence of catalyst

Question 26

properties of enzymes

Answer 26

speed up rxns by lowering the activation energy, highly specific for individual substrates/rxns (unique active sites), dont alter chemical rxn, and not permanently altered in chemical rxns

Question 27

Properties of water

Answer 27

high specific heat, carries heat with it when changing state, cushions/protects structures, acts a lubricant, primary solvent, dissolve hydrophilic substances

Question 28

high specific heat of water

Answer 28

water absorbs a high amount of heat without experiencing a significant temperature change itself; cells wont be damaged even when we are in hot temperatures

Question 29

why does water protect organs

Answer 29

high density of water (caused by hydrogen bonds) means that organs (less dense) are slightly suspended in water, reducing the weight of organs

Question 30

Water as a lubricant

Answer 30

reduces friction that occurs when 2 objects (organs) rub against one another (serous membranes)

Question 31

acid

Answer 31

hydrogen ion donor; when placed in water, it splits into the hydrogen cation (H+) and an anion; H+ gets donated to solution so the solutions concentration of H+ increases

Question 32

base

Answer 32

hydrogen ion acceptor (alkali); when placed in water, it dissociates and its anions bond with the excess H+ ions in the solution; low H+ concentration

Question 33

typical pH of blood

Answer 33

7.35

Question 34

Carbonic acid - Bicarbonate buffer system

Answer 34

H2CO3 <-> H+ + HCO3-; reversible reaction; resists large swings in pH by either bonding with excess H+ ions (R to L if solution is too acidic) or dissociating into H+ ions (L to R if solution is too basic); used for blood pH

Question 35

electrolytes

Answer 35

result from a salt (ionic bond) dissolving in water and dissociating into its cations and anions; the cations/anions in the solution are electrolytes; conduct current in water; all salts and some acids and bases form electrolytes