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Basic Chemistry > Unit 1: Essentials > Flashcards

Unit 1: Essentials Flashcards

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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
Q

electrolysis reaction

A

chemical method

Electrolysis: A process in which a nonspontaneous oxidation-reduction reaction is forced to occur upon passage of electric current thru a sample

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26
Q

hypothesis

A

Tentative explanation of a natural phenomenon

Must satisfy 2 criteria:

  1. testable
  2. falsifiable
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27
Q

kinetic energy

A

Energy of motion

The energy possessed by an object because of its motion

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28
Q

solute

A

The compound being dissolved

The lesser amount

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29
Q

heterogeneous mixture

A

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
Q

When is a chemical system most stable?

A

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
Q

scientific theory

A

A set of many observations collected under many different circumstances that agree with each other and provide a cohesive explanation of the physical world

* not proven, just hasn’t been disproven *

32
Q

potential energy

A

energy of position

33
Q

systemic error

A

Often caused by using instruments incorrectly and tend to skew the data in one direction

34
Q

nonmetals

A

An element that typically has a dull appearance and is a poor conductor of electricity

35
Q

energy

A

Capacity to do work or transfer heat

36
Q

atomic theory

A

The theory that all matter is made up of tiny indivisible particles (atoms).

Most important theory in Chemistry

37
Q

What is the reactant of a chemical reaction?

A

Left side of a chemical equation

A substance converted into another substance(s) during a chemical reaction

38
Q

falsifiable

A

A hypothesis has falsifiability if it can logially be proven false by contradicting it with a basic statement.

39
Q

metals

A

An element characterized by luster and the ability to conduct electricity

40
Q

chemical equation symbols

A

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
Q

dependent variable

A

The value that is measured

Plotted on y-axis (vertical)

42
Q

What is the product of a chemical reaction?

A

Right side of a chemical equation

A substance formed from another substance(s) during a chemical reaction

43
Q

aqueous solution

A

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
Q

pure substance

A

Matter that contains only 1 type of particle

Can’t be physically separated

45
Q

chemical formula

A

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
Q

Why is Chemistry called the central science?

A

It explains much of the world around us

Also bridges the gap between physics and biology

47
Q

quantitative

A

Numeric information

48
Q

precise

A

Measurements that agree with each other

Could all be right or wrong but they’re close to each other

49
Q

element

A

A pure substance that cannot be broken down to a more fundamental substance by a chemical method

EX: Hydrogen (H) or Oxygen (O)

50
Q

heat

A

Capacity to change something’s temperature

51
Q

instrument

A

A tool with the capacity to compare physical quantities

52
Q

compound

A

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
Q

molarity

A

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
Q

scientific inquiry

A

Asking and answering questions about the world according to the rules of the scientific method

55
Q

concentration

A

The relative amounts of solute and solvent in a solution

The amount of substance per amount of water (solvent) in an aqueous solution

56
Q

molecule

A

A single particle made from 2 or more atoms

2 or more elements bound together in a discrete arrangement

57
Q

scientific law

A

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
Q

composition

A

What matter is made of - the number and type of particles it contains

59
Q

mathematical and physical models

A

Representations of reality that allow us to predict behavior

Component of scientific theories

60
Q

intensive

A

Does not depend on amount

Density is an important property of matter because it is intensive

61
Q

Celsius

A

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
Q

physical properties

A

Describe what matter is like

Something that can be observed without altering the composition of the material

EX:

  • color
  • density
  • conductivity
  • mass
  • volume
63
Q

derived units

A

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
Q

moles

A

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
Q

experiment

A

A set of observations performed under controlled conditions that directly evaluate the merits of the hypothesis

66
Q

accurate

A

Measurements that are close to the true or expected value

67
Q

solvent

A

The substance doing the dissolving

The greater amount (e.g. water in an aqueous solution)

68
Q

slope

A

Slope of the trendline represents the constant of proportionality for the 2 variables

rise / run

change in y / change in x

69
Q

uncertainties in measurements

A

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
Q

independent variable

A

The value the experimenter controls

Plotted on x-axis (horizontal)

71
Q

testable

A

The claims the hypothesis makes can be evaluated with experient

Basic Chemistry (7 decks)

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