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Geometry, Chem > Unit 1 And 2 Chem > Flashcards

Unit 1 And 2 Chem Flashcards

1
Q

Scientific method

A

Define, observe, hypothesis, experiment, outcome of law or theory

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2
Q

Units of measurement

A

Tera, giga, mega, Kilo, hecto, deca, base, deci, centi, milli,, micro, nano, pico

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3
Q

Sig fig rules

A
  1. Non zeros significant
  2. Sandwiched zeros significant
  3. Numbers on right of decimal significant if number is greater than 1
  4. Zeros on left of decimal point of 1 insignificant
  5. Trailing zeros may/may not be significant
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4
Q

Volume of sphere

A

4/3 pi r (to the third power)

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5
Q

Volume of cylinder

A

Pi r(to second power) h

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6
Q

Volume of rectangle

A

Lwh

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7
Q

Density of Al

A

2.699g/cm3

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8
Q

Density of ethanol

A

0.789g/ml

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9
Q

How many quarts in a liter

A

1.06 quarts

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10
Q

How many cups in a quart(er)

A

4

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11
Q

How many oz in a lb

A

16

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12
Q

How many grams in Troy oz

A

31.103 grams

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13
Q

How many km in one mile

A

1.609 km

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14
Q

Pure substances

A

Matter with uniform composition and distinct properties

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15
Q

Mixture

A

Concentration of 2+ substances where each substance retains specific identities (heterogenous ex. Oil and water) (homogenous, composition is the same ex. Sand and iron filings)

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16
Q

Filtration

A

Removal of solids from liquids in solution

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17
Q

Distillation

A

Selective separation with condensation/evaporation

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18
Q

Chromatography

A

Separation/distribution of components in solution with mobile and stationary phase

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19
Q

Element

A

Substance that cannot be reduced or separated into a simpler substance, all identical atoms

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20
Q

Compound

A

Substance composed of 2+ elements chemically combined with fixed proportions, different elements chemically bonded together

21
Q

Physical properties

A

Can be measured without changing composition or identity of substance ex. Melting or boiling point

22
Q

Chemical properties

A

Measured through end result of chemical reaction ex. Hard boiling of egg, rusting, digesting, combustion

23
Q

Extensive property

A

Depends how much matter used ex. Mass, volume, length

24
Q

Intensive property

A

Does not matter how much matter used ex. Area, density, temperature, boiling point

25
Q

Atomic theory

A
  1. All elements are composed of atoms
  2. All atoms are identical in elements
  3. Compounds composed of atoms of 2+ elements in fixed ratio
  4. Chemical reactions can only separate, rearrange or combine
26
Q

Law of definite porportions

A

Fixed proportions regardless of sample size

27
Q

Law of multiple proportions

A

2 elements can form different compounds ex. H20 and h202

28
Q

Law of conservation of mass

A

Matter cannot be created or destroyed

29
Q

Atom

A

Basic unit of element that can enter into chemical combination

30
Q

Radiation

A

Emission and transmission of energy in forms of rays, discovered by JJ Thomson cathode ray tube experiment (determined ratio of electric charge to mass of electron)

31
Q

Robert milligan oil drop experiment

A

Determined actual charge of electrons when suspended by velocity

32
Q

Bequerel radioactivity

A

Discovered spontaneous emissions of particles & emission, alpha beta gamma

33
Q

Rutherford goil

A

-atom is mostly empty space, nucleus positively charged and is small and dense (observations that most alpha particles traveled through foil, some were deflected by small angles and few bounced back)

34
Q

Chadwick beryllium

A

Shot alpha rays at beryllium and discovered neutrons

35
Q

Atomic mass

A

(Atomic mass 1) (% as decimal) + (atomic mass 2) (% as decimal)

36
Q

Metal propeties

A

Good conductors of heat and electricity, all solid except mercury; some are magnetic, malleable, majority, mostly silver/green

37
Q

Mettalloids

A

Between metals and non metals chemically and geographically

38
Q

Non metals

A

Opposite of metals, all gas excluding bromine, varity of colors

39
Q

Alkali metals

A

Extremely explosive, stored under oil or argon capsules

40
Q

Alkaline earth metals

A

2 valence electrons, good conductors of electricity

41
Q

Transition metals

A

Form colored solutions

42
Q

Halogens

A

Always diatomic- must be in chemical bond, only group with all 3 phases

43
Q

Noble gasses

A

Inert, stable electron configuration of 8

44
Q

Molecule

A

2+ atoms in definite arrangement held by chemical covalent bonds ex. H2

Polyatomic molecules have 3+ atoms (can be same or different elemtents)

45
Q

Charged ion

A

Atom(s) w net positive/negative charge

46
Q

Binary compounds (ionic)

A
  • ide ending
47
Q

Ternary compounds (ionic)

A

Roman numerals, ide ending, ecspecially used with transition metals

48
Q

Covalent molecular naming prefixes

A

Mono di tri tetra penta hexa hepta octa Nona deca

49
Q

Acids

A

H+ ion
In binary acid use hydro prefix and ic ending w acid
In ternary acid no hydro prefix but add acid

Ate becomes ic, ite becomes ous

Oxyacids have “per” at beginning containing hydrogen and polyatomic ions with 02

Geometry, Chem (25 decks)

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