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Basic Chemistry > Unit 1: Essentials > Flashcards

Unit 1: Essentials Flashcards

1
Q

states of matter

A

Physical form of matter - solid, liquid or gas

Each phase has a distinct set of properties across a large number of compounds

Each phasee is different beause of the distance and interactions between their particles

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2
Q

dimensional analysis

A

A problem solving technique that allows us to convert measurements from one unit to another or from one quantity to another

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3
Q

base units of measurement

A

Unit Symbol__Quantity meter m length kilogram kg mass second s time Kelvin K temperature Celcius °C temperature mole mol amount of substance

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4
Q

chemical properties

A

How something will react

Defined by what chemical changes it can undergo; this will alter the composition of the material

EX:

  • flamability
  • resistance to rust
  • stability in water
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5
Q

matter

A

Anything that occupies space and has mass

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6
Q

composition of matter (decision tree)

A
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7
Q

work

A

Capacity to move something

The action of a force over a distance

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8
Q

Chemistry

A

The study of matter and the transformations it can undergo

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9
Q

random error

A

Caused by the factors beyond your control and can go in either direction

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10
Q

particles

A

A small portion of matter

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11
Q

What does a chemist do?

A

study matter

includes studying structure, symbols, nomenclature, properties, reactivity, calculations and lab skills

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12
Q

Fahrenheit

A

Measurement of temperature; most common in America

Symbol: °F

Water boils: 212°F

Room temp: 77°F

Ice melts / water freezes: 32°F

TF = 1.8 TC + 32

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13
Q

qualitative

A

Descriptive information

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14
Q

scientific method

A

A method of inquiry or investigation that involves cycles of observation and interpretation

A set of guidelines for skeptically investigating the world; it is “a way of trying not to fool yourself”

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15
Q

physical change

A

An experimental tehnique that does not alter the particles involved

Separate a mixture into its pure substances

EX: Solid carbon dioxide (dry ice) sublimes to make carbon dioxide gas

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16
Q

mixture

A

Matter that contains 2 or more types of particles

Can be physically separated

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17
Q

semimetals

A

AKA metalloid

An element that has properties intermediate between those of metals and nonmetals

An element with physial properties resembling a metal but chemical reactivity like that of a nonmetal

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18
Q

chemical change

A

Reaction

A process in which one or more substances are converted into new substances that have compositions and properties different from those of the original substance

EX: Methane burns in air (combusts) to produce water and carbon dioxide

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19
Q

atom

A

A single particle

One of the fundamental units of matter

The smallest particle of an element that retains the characteristic chemical properties of the element

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20
Q

diluted

A

Adding water to a concentrated sample

McVc = MdVd

M: molarity

V: volume

c: concetrated solution
d: diluted solution

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21
Q

homogenous mixture

A

Contains more than 1 type of particle but it has uniform composition throughout

EX: Salt water - water molecules with salt distributed uniformly throughout the entire sample

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22
Q

Kelvin

A

Measurement of temperature; most common in science

Has an absolute 0 - 0K is the coldest possible temperature

Symbol: K

Water boils: 373.15K

Room temp: 298.15K

Ice melts/water freezes: 273.15K

TK = TC + 273.15

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23
Q

electrical potential energy

A

Energy of charged particles near each other

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24
Q

density

A

Ratio of the object’s mass to its volume, usually reported in units of g/mL

d = m / v

Water has a density near 1 g/mL at room temp

Gases are lower - approx 10-3 g/mL

Solids are higher - up to 20 g/mL

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25
electrolysis reaction
chemical method ## Footnote Electrolysis: A process in which a nonspontaneous oxidation-reduction reaction is forced to occur upon passage of electric current thru a sample
26
hypothesis
Tentative explanation of a natural phenomenon Must satisfy 2 criteria: 1. testable 2. falsifiable
27
kinetic energy
Energy of motion The energy possessed by an object because of its motion
28
solute
The compound being dissolved The lesser amount
29
heterogeneous mixture
Contains more than 1 type of particle but is not uniform throughout EX: oil & vinegar dressing - contains distinct regions and is not uniform throughout
30
When is a chemical system most stable?
When they have minimized their potential energy Molecules form and reactions happen because they stablize the particles involved by minimizing their electrical potential energy
31
scientific theory
A set of many observations collected under many different circumstances that agree with each other and provide a cohesive explanation of the physical world ## Footnote **\* not proven, just hasn't been disproven \***
32
potential energy
energy of position
33
systemic error
Often caused by using instruments incorrectly and tend to skew the data in one direction
34
nonmetals
An element that typically has a dull appearance and is a poor conductor of electricity
35
energy
Capacity to do work or transfer heat
36
atomic theory
The theory that all matter is made up of tiny indivisible particles (atoms). Most important theory in Chemistry
37
What is the reactant of a chemical reaction?
Left side of a chemical equation A substance converted into another substance(s) during a chemical reaction
38
falsifiable
A hypothesis has _falsifiability_ if it can logially be proven false by contradicting it with a basic statement.
39
metals
An element characterized by luster and the ability to conduct electricity
40
chemical equation symbols
Reactant (left): original substances Product (right): new substances → produces or yeilds + reacts with / added to → (w/ delta above) heat is a catalyst for the reaction → (w/ Fe above) iron is a catalyst NR no reaction (s) solid or precipate (l) liquid (g) gas (aq) aqueous solution
41
dependent variable
The value that is measured Plotted on y-axis (vertical)
42
What is the product of a chemical reaction?
Right side of a chemical equation A substance formed from another substance(s) during a chemical reaction
43
aqueous solution
Homogeneous mixture between water and a soluble compound Not technically a state of matter but is so common that it's treated that way Symbol: (aq)
44
pure substance
Matter that contains only 1 type of particle Can't be physically separated
45
chemical formula
Atomic composition of a compound Communicates the elements involved using symbols from the periodic table and the relative numbers of those elements, using subscripts Molecular or covalent compounds ⇒ molecular formula Ionic compounds ⇒ formula units
46
Why is Chemistry called the central science?
It explains much of the world around us Also bridges the gap between physics and biology
47
quantitative
Numeric information
48
precise
Measurements that agree with each other Could all be right or wrong but they're close to each other
49
element
A pure substance that cannot be broken down to a more fundamental substance by a chemical method EX: Hydrogen (H) or Oxygen (O)
50
heat
Capacity to change something's temperature
51
instrument
A tool with the capacity to compare physical quantities
52
compound
A substance composed of 2 or more elements combined in definite proportions A pure substance that can be broken down further by a chemical method EX: Water (H2O) contains a single type of particle but can be broken down to Hydrogen and Oxygen
53
molarity
The number of moles of solute per liter of solution M = mol of solute / L solution Units: mol/L or M (molar) Symbol: M
54
scientific inquiry
Asking and answering questions about the world according to the rules of the scientific method
55
concentration
The relative amounts of solute and solvent in a solution The amount of substance per amount of water (solvent) in an aqueous solution
56
molecule
A single particle made from 2 or more atoms 2 or more elements bound together in a discrete arrangement
57
scientific law
A statement about nature that is always observed under a set of specific conditions Unlike a theory, it does not provide any explanation for its observations EX: conservation of mass, conservation of energy
58
composition
What matter is made of - the number and type of particles it contains
59
mathematical and physical models
Representations of reality that allow us to predict behavior Component of scientific theories
60
intensive
Does not depend on amount Density is an important property of matter because it is _intensive_
61
Celsius
Measure of temperature; most common outside America Symbol: °C Water boils: 100°C Room temp: 25°C Ice melts / water freezes: 0°C TC = (TF - 32)/1.8
62
physical properties
Describe what matter is like Something that can be observed without altering the composition of the material EX: * color * density * conductivity * mass * volume
63
derived units
Multiplying or dividing measurements with base units produces a new quantity with _derived units_. EX: Area (m2) or volume (m3) 1 mL = 1 cm3
64
moles
Concept introduced to make it more convenient to count atoms 1 mole of a substance contains 6.02 x 1023 particles (Avogadro's Number) Measure of the amount of a substance
65
experiment
A set of observations performed under controlled conditions that directly evaluate the merits of the hypothesis
66
accurate
Measurements that are close to the true or expected value
67
solvent
The substance doing the dissolving The greater amount (e.g. water in an aqueous solution)
68
slope
Slope of the trendline represents the constant of proportionality for the 2 variables rise / run change in y / change in x
69
uncertainties in measurements
There is error associated with every piece of scientific data ever collected No measurement is perfect 2 types of error: 1. random error 2. systemic error
70
independent variable
The value the experimenter controls Plotted on x-axis (horizontal)
71
testable
The claims the hypothesis makes can be evaluated with experient

Basic Chemistry (7 decks)

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