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Alexis Small > Chem 104- Unit 1 and 2 > Flashcards

Chem 104- Unit 1 and 2 Flashcards

1
Q

Scientific Method

A

approach to acquire knowledge through the observation of phenomena

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2
Q

Experiment

A

an observation of natural phenomena tested in a controlled and repeatable process and a rational conclusion can be made

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3
Q

hypothesis

A

a tentative and testable explanation for an observation or a series of observations

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4
Q

theory

A

a tested explanation of basic natural phenomena

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5
Q

law

A

a statement that summarizes a vast number of experimental observations, and describes or predicts some aspect of the natural world

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6
Q

measurements

A
  • essential for characterizing physical and chemical properties of matter
  • two parts: number and unit
  • standardization of the units of measurement is essential
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7
Q

Uncertainty in measurements

A

a digit that must be estimated is called uncertain (last recorded digit)

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8
Q

precision vs. accuracy

A

precision- agreement among repeated measurements
accuracy- agreement between a measured value and the accepted or true value

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9
Q

dimensional analysis

A

method for calculation where you carry along the units for quantities, a way to convert units from what you start with to what you need

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10
Q

chemistry

A

the study of the composition and structure matter and of the changes that matter undergoes

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11
Q

matter

A

whatever occupies space and can be perceived by our senses

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12
Q

mass

A

the quantity of matter

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13
Q

the law of conservation of mass

A

no mass is lost from the start of a process to the end

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14
Q

extensive vs. intensive properties

A

extensive (mass, volume, etc.)-> depends on the amount of substance
intensive (color, melting point, density)-> does not depend on the amount of subbstance

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15
Q

physical vs. chemical property

A

physical property (luster, hardness, color, etc.)-> can be observed without doing a chemical reaction
chemical property (flammability, reactivity)-> cannot be observed without doing a chemical reaction

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16
Q

pure substance

A
  • same physical and chemical properties throughout
  • cannot be separated into simpler substances by a physical process
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17
Q

mixture

A
  • combination of two or more pure substances
  • can be separated by physical processes
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18
Q

elements

A

a pure substance that cannot be separated into simpler substance by any chemical process (this includes diatomic and polyatomic molecules with only one element)

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19
Q

Common Diatomic and Polyatomic Molecules

A

“BrINClHOF”-> Br2, I2, N2, Cl2, H2, O2, F2
P4, S8

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20
Q

compound

A

pure substances composed to two or more different elements bonded together in fixed proportions (can be broken down into individual elements via chemical means)

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21
Q

The Law of Constant Composition/Law of Definite Proportions

A
  • all samples of a particular compound contain the same elements combined in the same proportions
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22
Q

Homogeneous

A

components are distributed uniformly throughout the sample and have no visible boundaries or regions

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23
Q

heterogeneous

A

components are not distributed uniformly, and there may be distinct regions with different compositions

24
Q

Separating Mixtures

A

Distillation, filtration, chromatography

25
Q

Nucleus

A

positively charged at the center of the atom, contains the vast majority of the atom’s mass (about 1/10,000 the size of the atom)

26
Q

nucleons

A

particles in the nucleus

27
Q

protons

A

positively charged subatomic particles, the atomic number

28
Q

neutrons

A

electrically neutral subatomic particles

29
Q

atomic mass units

A

units used to express the relative masses of atoms and subatomic particles
- equal to 1/12 the mass of a carbon-12 atom
- 1 amu = 1 Dalton

30
Q

group 1, 2, 17, 18, middle, bottom 2

A

1: alkali metals, 2: alkaline earth metals, 17: halogens, 18: noble gases, middle: transition metals, bottom 2: lanthanides, actinides

31
Q

metals

A
  • left side and bottom
  • shiny solids, conduct heat and electricity, are malleable
32
Q

nonmetals

A

right side and top of table
- solids, liquids, and gases, nonconductors, solids are brittle

33
Q

metalloids

A

between metals/nonmetals
- shiny solids, brittle, semiconductors

34
Q

atomic mass

A

total number of nucleons (protons and neutrons) in the nucleus
- upper left

35
Q

atomic symbol

A

a one or two letter symbol to identify the type of atom

36
Q

atomic number

A

the number of protons in the nucleus, determines the identity of the element
- bottom left

37
Q

isotopes

A

atoms of the same element that contains a different number of neutrons, and thus has a different atomic mass

38
Q

average atomic mass

A

weighted average of the masses of ALL isotopes of an element (different than a normal average which assumes equal contribution from each piece)

39
Q

natural abundance

A

proportion of a particular isotope, usually expressed as a percentage, that is found for that element in natural samples

40
Q

how to calculate average atomic mass

A

weighted average = (mass of isotope 1)(abundance of isotope 1) + (Mass of Isotope 2)(Abundance of Isotope 2) + …

41
Q

ions

A
  • neutral atoms that gain/lose electrons become ions
  • ions are held together by electrostatic force (opposites attract)
42
Q

cations vs anions

A

cations = ions with positive charges
anions = ions with negative charges

43
Q

ionic compounds

A
  • metal and a nonmetal
  • metals form cations, nonmetals form anions
  • charges depend on locations in the periodic table
44
Q

formula unit

A

smallest electrically neutral unit of an ionic compound

45
Q

molecular compounds

A

composed of atoms held together in molecules by covalent bonds and are composed of nonmetals

46
Q

covalent bonds

A

bond between two atoms created by sharing one or more pairs of electrons

47
Q

molecular formula

A

shows the number and type of atoms present in one molecule of a compound

48
Q

empirical formula

A

shows the smallest whole-number ratio of elements in a compound

49
Q

naming binary molecular compounds

A

compounds consisting of two nonmetals
- first element in the formula is named first
- second element name is changed by adding the suffix “-ide”
- add prefixes to identify quantity of atoms
(mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca)

50
Q

rules for using prefixes

A
  • only use prefixes to indicate amount for molecular compounds
  • do not use the prefix mono when naming the first element
  • prefixes ending with o- and a- are modified when used with elements beginning with vowels
51
Q

binary ionic compounds

A

consist of cations (usually metals) and anions (usually nonmetals)

52
Q

naming binary ionic compounds

A
  • cation is named first, using the name of the element
  • anion is named second, adding the -ide suffix to the name of the element
  • never named based on amount, must always be neutral
  • for cases with multiple charges, we must include the charge in the name
53
Q

polyatomic ions

A

charged group of two or more atoms joined together by covalent bonds

54
Q

oxoanions

A

polyatomic anions containing oxygen in combination with one or more elements

55
Q

helpful rules for polyatomic ion naming

A
  • group ions together that have no prefix and end in -ate
  • when comparing similar ions, the ion ending in -ite has one less oxygen than -ate
  • adding the prefix per- to an ion ending in -ate means there is one more oxygen
  • adding the prefix hypo- to an ion ending in -ite means there is one less oxygen
56
Q

binary acids

A
  • contain hydrogen and a monoatomic anion
  • most common binary acids contain halogens
57
Q

naming binary acids

A
  • the prefix hydro- + the halogen base name + the suffix -ic + the word acid

Alexis Small (19 decks)

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