Unit 1

Front 1

sub atomic particle

Back 1

particles that make up an atom, i.e. protons, neutrons and electrons

Front 2

atom

Back 2

basic unit of an element, consists of nucleus, orbital and subatomic particles

Front 3

compound

Back 3

also called mixture, composed of two or more separate elements i.e. NaCl

Front 4

molecules

Back 4

group of atoms bonded together, smallest chemical compound that can take part in a reaction

Front 5

macromolecules

Back 5

commonly made through polymerization of smaller subunits, i.e. protein made of subunit amino acid

Front 6

organelles

Back 6

structure within a cell that have specific functions

Front 7

tissues

Back 7

materials that make up an organism i.e. muscle

Front 8

organs

Back 8

part of organism that is self contained and has a vital function i.e. liver

Front 9

organ system

Back 9

group of organs that work together to perform one or more functions i.e. skeletal system

Front 10

individual

Back 10

single organism

Front 11

population

Back 11

all that inhabit a specific area

Front 12

community

Back 12

group of people living in the same place or sharing a common characteristic

Front 13

ecosystem

Back 13

biological community

Front 14

biosphere

Back 14

regions of surface, hydrosphere and atmosphere

Front 15

carbon

Back 15

can have 4 covalent bonds, can bond to itself without turning into a gas

Front 16

alkane vs alkyne vs alkene and formulas

Back 16

alkane = single bonds (CnH2n+2)

alkene= double bonds (CnH2n)

alkyne = multiple bonds (CnH2n-2)

Front 17

cytoplasm

Back 17

gel like substance, surrounds all organelles

Front 18

mitochondria

Back 18

sausage shaped organelle, surrounded by double membrane, power house (glucose into ATP)

Front 19

cristae

Back 19

highly folded inner membrane of mitochondria , increases rates of energy transformation

Front 20

chloroplast

Back 20

double membrane, composed of stacks of granum, site for photosynthesis

Front 21

granum

Back 21

stacks of thylakoids, in chloroplast

Front 22

cellulose

Back 22

makes up cell wall in plants

Front 23

chromosomes

Back 23

keep DNA tightly packed around proteins

Front 24

nucleotide

Back 24

made of sugar, phosphate group and base, building block of RNA and DNA

Front 25

plasma membrane

Back 25

outer: isolates cell contents

inner: plays role in energy transformation

Front 26

phospholipid

Back 26

contains hydrophobic tails and hydrophilic head, makes up bilayer in cell membrane

Front 27

atomic number

Back 27

number of protons

Front 28

mass number

Back 28

sum of protons and neutrons

Front 29

bohr rutherford

Back 29

discovers nucleus and electrons surrounding it

Front 30

elements are arranged in what order on the periodic table

Back 30

increasing atomic number

Front 31

isotope

Back 31

atoms of an element with same atomic number but different mass number (diff number of neutrons)

Front 32

rutherford and brooks

Back 32

discover that nucleus of isotopes can decay.. radioisotopes release radioactivity

Front 33

radioactivity

Back 33

formation of different elements.. releases subatomic particles.. releases radiation

Front 34

which carbon isotope is radioactive?

Back 34

c-14

Front 35

what is half-life.. provide formula

Back 35

time for 1/2 of the atoms in a sample to decay ... A = Ao (1/2) ^t/h

Front 36

radioactive tracers

Back 36

radioisotopes used to follow chemicals through reactions .. trace their path as they move through cells in body

Front 37

radiolabelled molecules

Back 37

molecules containing specific radioisotopes.. used in nuclear medicine i.e. thyroid gland absorbs iodine.. can show size of gland on xrays

Front 38

can radiation be harmful

Back 38

high energy radiation can result in damaged cells and tissues.. can cause radiation sickness, mutation and cell death

Front 39

orbitals

Back 39

volume of space around the nucleus where electrons are found

Front 40

what is special about noble gases

Back 40

they don't try to lose or gain electrons

Front 41

what are the two main intramolecular forces? which is stronger?

Back 41

ionic (cation + anion) and covalent (sharing of electrons).. covalent is stronger

Front 42

electronegativity

Back 42

atoms ability to attract a pair of electrons in a covalent bond

Front 43

what electronegativity numbers show the polarity of a molecule?

Back 43

0 = non polar cov.

0.5 = polar covalent

1.7 = ionic

Front 44

hybridization

Back 44

when atoms react and form covalent bonds... their valence electrons change orientation

Front 45

ronald j gillespie

Back 45

VSEPR.. valence electrons repel each other ... results in special shapes

Front 46

what two factors affect the polarity of a molecule

Back 46

bond types and shape

Front 47

how do living cells resist changes in pH.. what are the common forms in humans?

Back 47

buffers: chemical systems containing substances that can donate H ions and remove them to neutralize pH (made up of conjugate acid and base pairs at equilibrium).. humans have carbonic acid and bicarbonate

Front 48

explain what happens in your blood when you eat a lemon (or something very acidic)

Back 48

H ions enter the blood from the food, HCO3 ions react with H ions, carbonic acid is produced making blood pH more basic

Front 49

what pH is blood supposed to be? what pH is fatal?

Back 49

around 7.4 .. increase or decrease of 0.2-0.4 can be fatal

Front 50

acidosis vs alkalosis

Back 50

acidosis = pH below 7.35

alkalosis = pH above 7.45

Front 51

what's an example of protein buffers in human body

Back 51

hemoglobin.. maintains pH of red blood cells

Front 52

what does water do in human body

Back 52

helps control body temp, protects brain and spinal cord

Front 53

what does the polarity of water allow

Back 53

ability to form chemical bonds with molecules and ions.. including itself

Front 54

how are intermolecular bonds broken

Back 54

solid to liquid and liquid to gas

Front 55

which are weaker.. intermolecular forces or intramolecular?

Back 55

intermolecular are weaker

Front 56

what are vanderwaals forces

Back 56

intermolecular forces..

1) london dispersion (weakest) - temporary unequal distribution of electrons

2) dipole-dipole - holds polar molecules together.. partial positive and partial negative

3) hydrogen bonds (strongest) - dipole-dipoles that only form between hydrogen and N, O or F

Front 57

what happens when ionic solids dissolve

Back 57

anion and cations dissociate (ionic bonds break)

Front 58

soluble

Back 58

substance that dissolves in other substances

Front 59

miscible vs immiscible

Back 59

miscible: liquids that dissolve into one another

immiscible: liquids that don't i.e. oil and water

Front 60

protein carriers

Back 60

help small molecules move in body bc they cannot form H bonds with water

Front 61

cohesion

Back 61

water spider.. clings bc h bonds to other water molecules.. increases surface tension

Front 62

adhesion

Back 62

water up tube.. h bonds with tube molecules.. capillary action

Front 63

high specific heat capacity of water

Back 63

moderates temp. bc the h bonds allow it to absorb heat

Front 64

high heat of vaporization of water

Back 64

absorbs heat.. sweat.. cool via evaporation

Front 65

why water is less dense as a solid

Back 65

crystal lattice and h bonds spread below 0°C

Front 66

autonization of water

Back 66

water donates an H ion .. creates OH and H3O .. neutralizes pH

Front 67

acid properties

Back 67

blue litmus red.. sour.. electricity

Front 68

base properties

Back 68

red litmus blue.. slippery.. bitter.. electricity

Front 69

neutralization

Back 69

when H and OH ions react to form water.. produces a salt and water

Front 70

do weak or strong acids and bases reach equilibrium

Back 70

weak bc strong ionize completely

Front 71

bronsted lowry acid-base theory

Back 71

reversible acid-base reactions involve transfer of protons

Front 72

conjugate acid vs conjugate base

Back 72

conj. acid: H added

conjugate base: H lost

Front 73

frederick wohler

Back 73

prepares urea by heating ammonium cyanate.. shows that idea "organic compounds can only be produced by living organisms" is false.... creates synthetic organic chemistry

Front 74

bonding capacity

Back 74

number of covalent bonds with adjacent atoms

Front 75

what functional groups do amino acids contain

Back 75

carboxyl (acidic) and amino (basic)

Front 76

polymers

Back 76

long chains of smaller subunits

Front 77

state the subunit of the following polymers:

1) starch

2) triglycerides

3) protein

4) DNA/RNA

Back 77

1) sugar (glucose)

2) glycerol and fatty acids

3) amino acids

4) nucleotides

Front 78

other name for condensation reaction and what is it

Back 78

dehydration synthesis.. creates covalent bond between two subunits .. removes OH from one and H from other .. water is produced

Front 79

anabolic vs catabolic reactions

Back 79

anabolic: construction of large form subunits

catabolic: break macros into subunits

Front 80

difference bw condensation reaction and hydrolysis

Back 80

condensation absorbs nrg.. hydrolysis releases energy

Front 81

hydrolysis

Back 81

water is used to break covalent bonds

Front 82

enzymes

Back 82

structures that recognize covalent bonds that must be created or broken

Front 83

biological catalysts

Back 83

speed up reactions without being consumed

Front 84

function of carbs

Back 84

energy, building material, cell identification, communication

Front 85

ratio of hydrogen to carbon to oxygen in carbs

Back 85

C:H:O = 1:2:1

Front 86

how are monosacharides names

Back 86

based on carbonyl group (al or one) and number of carbons in backbone

Front 87

what are the two simplest monosaccharides

Back 87

dihydroxyacetone and glyceraldehyde

Front 88

two examples of pentose sugars

Back 88

ribose and ribulose

Front 89

isomer and examples

Back 89

same chemical formula with different arrangement of atoms.. i.e. glucose, galactose and fructose

Front 90

what is special about monosaccharides with 5 or more carbons

Back 90

rings when dissolved in water but linear when dry

Front 91

what is special about glucose's 6 carbon ring

Back 91

there's a 50% chance the hydroxyl group at C1 will be below the ring (alpha glucose) and 50% chance it'll be above (beta glucose)

Front 92

what links do oligosaccharides have

Back 92

glycosidic (form by condensation).. H of one and OH of another form water