Leh Topic 3

Front 1

matter

Back 1

anything that takes up space and has mass

Front 2

atom

Back 2

the most basic unit of matter; the smallest particle that still maintains the most basic properties of a particular chemical element

Front 3

element

Back 3

a substance made up of all the same type of atom and cannot be broken down into other substances by physical or chemical means

Front 4

majority of living matter's elements

Back 4

Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorous

or CHONP

Front 5

protons

Back 5

positively charged

found in nucleus

mass = 1 amu

Front 6

neutrons

Back 6

neutrally charged

found in nucleus

mass = 1 ammu

Front 7

electrons

Back 7

negatively charged

found surrounding the nucleus in orbitals

mass = 1/1836 amu (negligible)

Front 8

amu

Back 8

atomic mass unit

Front 9

periodic table of elements

Back 9

organized according to atomic number

nonmetals on right and hydrogen

metals on left

semimetals in between metals and nonmetals

nobal gases group 18

each column is a group which contains elements that have similar chemical and physical properties

each row is a period

Front 10

atomic number

Back 10

the number of protons- IDENTITY, NEVER CHANGES

Front 11

mass number

Back 11

the number of protons and neutrons

Front 12

ion

Back 12

an atom that is not neutral; a charged particle as a result from an atom gaining or losing 1 or more electrons when reacting

Front 13

element symbolization

Back 13

symbol of element

mass number top left

atomic number bottom left

Front 14

isotopes

Back 14

atoms of the same element that have a different number of neutrons

Front 15

radioactive isotopes

Back 15

are because their nucleus is very unstable, so they disintegrate spontaneously, releasing radioactive particles

can be used to date fossils

are noted by their element and then their mass number (ex: carbon-14 for 6 protons and 8 neutrons)

Front 16

tracer elements

Back 16

radioactive isotopes used to label compounds in certain biological processes and chemical reactions which allows scientists to follow how a biological process occurs

O-18 is used to trace water in photosynthesis reactions

Front 17

electrons in the furthest energy level shell

Back 17

contain the most energy

Front 18

valence electrons

Back 18

electrons in the outermost energy levels

are the only electrons involved in chemical reactions to form ions and molecules

Front 19

inner electron shell

Back 19

can only hold 2 electrons

Front 20

outer electron shells

Back 20

can hold 8 electrons

Front 21

compound

Back 21

a pure substance made up of two or more different types of atoms chemically bonded together

ex: NaCl

Front 22

molecule

Back 22

a substance made up of two or more atoms which can be the same or different covalently bonded together

ex: CO2, or any of the diatomic elements

Front 23

diatomic elements

Back 23

H, O, F, Br, I, N, Cl; are commonly bonded together to create molecules

Front 24

glucose

Back 24

C6 H12 O6

Front 25

stability of atoms

Back 25

most stable when their valence or outermost shell is completely filled with electrons

this means 8 in most atoms, but 2 in Helium and Hydrogen

Front 26

atoms that are completely filled are

Back 26

stable and inactive (inert) (because they are content, dont need more or less electrons)

Front 27

the noble gases

Back 27

group 18 on the periodic table; are stable and unreactive

Front 28

chemical bond

Back 28

atoms giving up, sharing, or taking electrons from/with other atoms

Front 29

ions

Back 29

atoms that become charged as a result of losing or gaining electrons

Front 30

results of bonding of atoms

Back 30

molecules, compounds, or diatomic elements

Front 31

atoms that gain electrons

Back 31

become negatively charged ions, or anions

Front 32

atoms that lose electrons

Back 32

become positively charged ions, or cations

Front 33

ionic bond

Back 33

is the electrical attraction that holds oppositely charged ions together

this attraction results due to a transfer of electrons from one atom to another

usually exist between a metal and a nonmetal

ex: NaCl

Front 34

covalent bonding

Back 34

chemical bonding that is due to sharing electrons between atoms

typically occurs between two nonmetals

Front 35

single bonds

Back 35

covalent bond where 1 pair of electrons are shared, or 2 electrons

written as x - y

Front 36

double bonds

Back 36

covalent bond where 2 pairs of electrons are shared, or 4 electrons

written as x = y

Front 37

triple bonds

Back 37

covalent bond where 3 pairs of electrons are shared, or 6 electrons

written as x ≡ y

Front 38

saturated

Back 38

covalent bonds that have all single bonds

(is called saturated because the carbon is completely surrounded by bonds)

Front 39

unsaturated

Back 39

at least one double or triple bond

(is called because the carbon is not completely surrounded by bonds

Front 40

carbon can form

Back 40

4 covalent bonds

Front 41

electronegativity

Back 41

every atom has a different attraction for electrons

Front 42

polar molecules

Back 42

(puller = polar)

molecules whose atoms are covalently bonded, but have an unequal charge distribution (due to unequal electron pulling) resulting in oppositely charged poles

Front 43

nonpolar molecules

Back 43

(nonpuller = nonpolar)

molecules whose atoms are covalently bonded, but have an equal charge distribution (due to equal electron pulling) resulting in uncharged poles

Front 44

intermolecular foces

Back 44

forces of attraction that exist between molecules

Front 45

hydrogen bonding

Back 45

bonding between the partial positive hydrogen of one molecule and the partial negative O, N, or FL of another molecule

this bong is strong compared to other intermolecular forces but weak compared to forces of attraction that exist within a molecule

Front 46

special function of hydrogen bonding

Back 46

keeps two strands of DNA bonded together, forming a double helix

Front 47

structural and chemical characcteristics of water

Back 47

are responsible for many of waters unique properties

Front 48

properties of water

Back 48

has a high specific heat capacity

has a high heat of vaporization

is the universal solvent

has molecules that are both adhesive and cohesive

solid form (ice) floats on it's own liquid form (liquid water)

Front 49

specific heat capacity

Back 49

the amount of heat energy needed to raise 1 gram of a substance 1 degree Celsius

since waters specific heat capacity is high this means it takes a lot of heat energy to raise the temperature of water

this allows internal stability for many organisms (homeostasis), makes large bodies of water stable environments, and allows coastal areas to experience moderate climates because of ocean moderation

Front 50

heat of vaporization

Back 50

the amount of heat needed to convert 1 gram of a substance from liquid to gas

since waters heat vaporization is high, it takes a lot of heat energy to convert liquid water in water vapor

this gives animals an efficient way to lower their body temperature when it gets too high (sweating)

Front 51

solute

Back 51

a substance that dissolves in another substance

Front 52

solvent

Back 52

the substance that dissolves a solute

Front 53

since water is highly polar,

Back 53

it has the capacity to dissolve all other polar and ionic substances

Front 54

hydrophilic

Back 54

means waterloving or attracted to water

polar and ionic substances are this

Front 55

hydrophobic

Back 55

means water fearing or repelled by water

nonpolar substances at this

Front 56

dissolving tips/hints

Back 56

"like dissolves like"

nonpolar substances only dissolve other nonpolar substances

while

polar substances only dissolve other polar or ionic substances

Front 57

biological significance of water being the universal solvent

Back 57

table salt (NaCl) and ammonia (NH3) dissolve easily in polar water

oil (mainly nonpolar compounds) and CO2 (nonpolar) does not dissolve well in polar water

Front 58

adhesion

Back 58

the clinging of one substance to another substance

Front 59

cohesion

Back 59

the clinging of a substance to other molecules of itself

Front 60

biological significance of water being both adhesive and cohesive

Back 60

adhesion causes the formation of a meniscus along the side of a container

cohesion results in waters high surface tension which allows insects to walk on water

both forces working together allow water to defy gravity and flow up a narrow "path" (like a plant stem) (capillary action)

Front 61

transpiration

Back 61

evaporation on the leaves of plants

Front 62

density

Back 62

the mass of an object per unit volume

Front 63

solid ice is

Back 63

less dense than liquid water since water has the unique property in which its molecules spread out farther from one another in the solid form than in the liquid form

this allows aquatic life to live and survive under the ice in the winter, since ice floats, then warm water is near the surface, and the colder water is at the bottom of an ocean