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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
Nucleus
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
nucleons
particles in the nucleus
27
protons
positively charged subatomic particles, the atomic number
28
neutrons
electrically neutral subatomic particles
29
atomic mass units
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
group 1, 2, 17, 18, middle, bottom 2
1: alkali metals, 2: alkaline earth metals, 17: halogens, 18: noble gases, middle: transition metals, bottom 2: lanthanides, actinides
31
metals
- left side and bottom - shiny solids, conduct heat and electricity, are malleable
32
nonmetals
right side and top of table - solids, liquids, and gases, nonconductors, solids are brittle
33
metalloids
between metals/nonmetals - shiny solids, brittle, semiconductors
34
atomic mass
total number of nucleons (protons and neutrons) in the nucleus - upper left
35
atomic symbol
a one or two letter symbol to identify the type of atom
36
atomic number
the number of protons in the nucleus, determines the identity of the element - bottom left
37
isotopes
atoms of the same element that contains a different number of neutrons, and thus has a different atomic mass
38
average atomic mass
weighted average of the masses of ALL isotopes of an element (different than a normal average which assumes equal contribution from each piece)
39
natural abundance
proportion of a particular isotope, usually expressed as a percentage, that is found for that element in natural samples
40
how to calculate average atomic mass
weighted average = (mass of isotope 1)(abundance of isotope 1) + (Mass of Isotope 2)(Abundance of Isotope 2) + ...
41
ions
- neutral atoms that gain/lose electrons become ions - ions are held together by electrostatic force (opposites attract)
42
cations vs anions
cations = ions with positive charges anions = ions with negative charges
43
ionic compounds
- metal and a nonmetal - metals form cations, nonmetals form anions - charges depend on locations in the periodic table
44
formula unit
smallest electrically neutral unit of an ionic compound
45
molecular compounds
composed of atoms held together in molecules by covalent bonds and are composed of nonmetals
46
covalent bonds
bond between two atoms created by sharing one or more pairs of electrons
47
molecular formula
shows the number and type of atoms present in one molecule of a compound
48
empirical formula
shows the smallest whole-number ratio of elements in a compound
49
naming binary molecular compounds
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
rules for using prefixes
- 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
binary ionic compounds
consist of cations (usually metals) and anions (usually nonmetals)
52
naming binary ionic compounds
- 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
polyatomic ions
charged group of two or more atoms joined together by covalent bonds
54
oxoanions
polyatomic anions containing oxygen in combination with one or more elements
55
helpful rules for polyatomic ion naming
- 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
binary acids
- contain hydrogen and a monoatomic anion - most common binary acids contain halogens
57
naming binary acids
- the prefix hydro- + the halogen base name + the suffix -ic + the word acid

Alexis Small (19 decks)

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