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Science 10 > Chem 10 vocab > Flashcards

Chem 10 vocab Flashcards

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1
Q

Alkali metals

A
  • group 1
  • soft, shiny and silver
  • very reactive with water
  • reactivity increases as you move down the group
  • their compounds are soluble in water
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2
Q

Alkaline Earth Metals

A
  • group 2
  • shiny, silver, but not as soft as group 1
  • form oxide coatings when exposed to air
  • coumpounds are white, but less soluble than group 1
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3
Q

anion (-)

A
  • formed when non-metals gain electrons
  • negatively charged
  • charge = number of electrons that are gained (- = 1 was gained)
  • change to “ide” (chlorine atom -> chloride ion)
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4
Q

Atom

A

smallest part of an element with properties of an element.

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5
Q

atomic number

A

number of protons and electrons

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6
Q

Bohr Model

A

Each energy level has a max number of electrons that can reside in it, and they can jump from one level to another. Electrons travel in seperate orbits and are attracted to the nucleus.

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7
Q

cation (+)

A
  • formed when metal atoms lose electrons
  • positively charged
  • charge = the number of electrons that were lost (+ = 1 lost)
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8
Q

chemical change

A

a change that is permanent (evidence of gas, precipitate, heat, light)

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9
Q

compound

A

A combination of two or more elements

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10
Q

Dalton model

A

stated that all matter is composed of atoms that can’t be created or destroyed into smaller particles. All atoms of an element are identicle.

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11
Q

Element

A

Made of atoms and cannot be broken

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12
Q

energy level

A

region of space where electrons are found

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13
Q

group

A
  • columns
  • number of electrons on outermost layer (valence) = group number
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14
Q

Halogens

A
  • group 17
  • elements are poisonous
  • react with alakali metals to form salt
  • reactivirty increases as you move up the group
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15
Q

heterogeneous mixture (mechanical mixture)

A

A mixture where you can see the parts

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16
Q

homogeneous mixture

A

a unifrom mixture, usually a liquid (iced tea, chocolate milk)

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17
Q

ion

A
  • electricaly charged atom or group of atoms
  • do not have an equal amount of protons and electrons
  • more protons = positive charge
  • more electrons = negative charge
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18
Q

ionic compound properties

A
  • have high melting points
  • retain crystal shapes (lattice)
  • are soluble in water
  • are conductors - are electrolytes
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19
Q

isotope

A

atom of an element with a different number of neutrons from protons

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20
Q

mass number

A

number of protons + number of neutrons

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21
Q

metalloids

A
  • solids and gasses
  • between non-metals and metals
  • some can conduct
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22
Q

Metals

A
  • most are shiny and grey
  • malleable and ductile
  • conducts
  • solids at room temperature (except mercury)
  • forms cations (+ ions)
  • on left side of staircase
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23
Q

mixture

A

two or more substances combined

24
Q

molecular compound properties

A
  • low melting points
  • crumble easily (don’t maintain crystal lattice)
  • most are not soluble in water
  • low or no conductivity - not an electrolyte
25
Q

Noble gases

A
  • group 18
  • are unreactive
26
Q

non-metals

A
  • can be L, S, or G at room temp
  • some highly reactive and some unreactive
  • form anions (- ions)
  • right side of staircase
  • vary in color and dull
  • poor conductors
  • not malleable, and are brittle
27
Q

number of neutrons can be calculated…

A

mass number - number of protons

28
Q

octet rule

A

atoms gain or lose electrons to have a full valence shell.
* a transfer of electrons occur from the metal to the non-metal

29
Q

Period

A
  • rows
  • the number of energy levels occupied by electrons = period number
30
Q

physical change

A

a change in form that is reversable (H2O melting to freezing)

31
Q

Pure Substance

A

It has one type of particle (anything on periodic table)

32
Q

Quantum Mechanical model

A
  • today’s model of the atom
  • Electrons exist in the cloud of negative that surrounds the nucleus
  • nucleus contains the protons (+) and neutrons (0)
33
Q

Rutherford Model

A

Hypothesized that the atom is mainly empty space but each atom has a small positively charged core (nucleus). Nucleus accounts for majourity of the atom’s mass.

34
Q

suspension

A

a heterogeneous mixture that settles

35
Q

Thompson Model

A

Accounted for the existence if small negative charges, and these electrons have shells or energy levels.

36
Q

transition metals

A

these elements have a wide range of chemical and physical properties.

37
Q

water polarity

A

one end is negative and the other is positive.
* has a higher boiling point because of its polarity
* negative oxygen and one positive hydrogen

38
Q

acid

A

coumpoud that dissolves in water to form a solution with a pH less than 7

39
Q

base

A

a compound that dissolves to form a solution with a pH greater than 7

40
Q

buffer

A

a substance that can keep a pH constant, even if an acid or base is added

41
Q

Acid properties

A
  • sour
  • not slippery
  • corrodes metal
  • litmus turns red
  • conducts
  • under 7 pH
42
Q

base properties

A
  • bitter
  • slippery
  • doesn’t corrode metal
  • litmus turns blue
  • conducts
  • over 7 pH
43
Q

neutralization

A
  • when acids and bases react together, both acid and basic properties dissapear
  • this reaction produces water and salt
44
Q

chemical reaction

A
  • formation of a gas
  • formation of precipitate
  • color change
  • energy change (heat, light, electricity)
45
Q

Endothermic

A

reactions that absorb energy

46
Q

exothermic

A

reactions that release energy

47
Q

enzyme

A

chemicals that speed up a reaction but are not used up by it

48
Q

law of conservation of mass

A

the totoal mass of all the reactants is equal to the total mass of all the products

49
Q

formation reaction

A

two element combine to form a compound
A + B = AB

50
Q

decomposition reactions

A

breaking a product down into it’s reactants (opposite of formation reaction)
AB = A + B

51
Q

(hydrocarbon) Combustion

A

CxHy + O2 = CO2 + H20
(usually burning)

52
Q

single replacement reaction

A

a reactive compound reacts with an element
A + BC = B + AC
non-metals trade places

53
Q

double replacement reaction

A

2 ionic compounds react (ususally occur in solutions)
AB + CD = AD + CB

54
Q

find mass

A

m = nxM

55
Q

find molar mass

A

M = m/n

56
Q

find moles

A

n = m/M

57
Q

covalent bonds

A

when atoms share electrons
* this happens in order to fill the valence shell (full octet)

Science 10 (2 decks)

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