Chemistry Ch. 1-3

Front 1

Chemistry

Back 1

the study of the composition and properties of matter

Front 2

Chemical reactions

Back 2

the way substances change when interacting with one another; transformations that alter the chemical compositions of substances

Front 3

Scientific method

Back 3

A cyclical process in which we gather and assemble information about nature, formulate explanations for what we've observed, and then test the explanations with new experiments

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Observation

Back 4

A statement that accurately describes something we see, hear, taste, feel, or smell

Front 5

Conclusion

Back 5

A statement that's based on what we think about a series of observation

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Data

Back 6

Observations we make while performing experiments

Front 7

Scientific Law

Back 7

A broad generalization that is based on the results of many experiments and is uniformly applicable to all of them

Front 8

Theoretical Models

Back 8

Mental pictures that can include hypotheses

Front 9

Hypotheses

Back 9

Tentative explanations

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Theory

Back 10

A tested explanation of the behavior of nature

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Atoms

Back 11

Tiny particles that make up all chemical substances (and all matter)

Front 12

Molecules

Back 12

When individual atoms combine in diverse ways to form more complex particles

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Mass

Back 13

Refers to how much matter there is in a given object

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Weight

Back 14

Refers to the force with which the object is attracted by gravity

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Decomposition

Back 15

When one substance is changed into two or more others

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Elements

Back 16

Substances that cannot be decomposed into simpler materials by chemical reactions

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Chemical Symbol

Back 17

An abbreviation of an element's name

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Compound

Back 18

A substance formed from tow or more differnt elements in which the elements are always combined in the same fixed proportions by mass

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Pure substances

Back 19

The composition of a pure substance is always the same, regardless of its source

Front 20

Mixtures

Back 20

Can have variable compositions

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Homogeneous Mixture

Back 21

Has the same properties throughout the sample

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Solution

Back 22

A type of homogeneous mixture

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Heterogeneous Mixture

Back 23

A mixture that consists of two or more regions, called phases, that differ in properties

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Physical Change

Back 24

When substances are mixed together, but no new chemical substances form

Front 25

Chemical Change

Back 25

When substances are mixed together and there is a change in the chemical makeup of the substances that are involved

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Physical Property

Back 26

A property that can be observed without changing the chemical makeup of a substance

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States of Matter

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Solids, liquids, and gases

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Extensive Property

Back 28

A property that depends on sample size

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Intensive Property

Back 29

A property that DOES NOT depend on sample size; for example, color, melting point, and boiling point

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Qualitative Observations

Back 30

Do not involve numerical information and are usually of limited value

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Quantitative Observations (Measurements)

Back 31

Do yield numerical data

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International System of Units (SI)

Back 32

The dominant system of units in science and engineering

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Base Units

Back 33

Length: meter
Mass: kilogram
Time: second
Electric current: ampere
Temperature: kelvin
Amount of substance: mole
Luminous intensity: candela

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Uncertainties (Errors)

Back 34

How measurements are inexact

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Accuracy

Back 35

Refers to how close a measurement is to the true or correct value

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Precision

Back 36

Refers to how closely rpeated measurements of a quantity come to each other and to the average

Front 37

Density

Back 37

The ratio of an objects mass to its volume

Front 38

Law of Conservation of Mass

Back 38

The mass of all reactants in a chemical reaction will be the same as the mass of the products

Front 39

Law of Definite Proportions

Back 39

In a given chemical compound, the elements are always combined in the same proportions by mass

Front 40

Dalton's Atomic Theory

Back 40

1. Matter consists of tiny particles called atoms.

2. Atoms are indestructible. In chemcial reactions, the atoms rearrange but they do not themselves break apart.

3. In any smaple of a pure elements, all the atoms are identical in mass and other properties.

4. The atoms of different elements differ in mass and other properties.

5. When atoms of different elements combine to form compounds, new and omre complex particles form. However, in a given compund the constituent atoms are always present in the same fixed numerical ratio.

Front 41

Law of Multiple Proportions

Back 41

Whenever two elements form more than one compound, the different masses of one elemnet that combine with the same mass of the other element are in the ratio of small whole numbers.

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Subatomic Particles

Back 42

The particles that atoms are composed of

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Protons

Back 43

Positive particles that are found in the nucleus of an atom

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Neutron

Back 44

Particles that are found in the nucleus of an atom; have no charge

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Electron

Back 45

Negative particles that are found in electron cloud, which surrounds the nucleus of an atom

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Nucleus

Back 46

The small, dense core of an atom

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Nucleons

Back 47

Sometimes used as a name for protons and neutrons since they are found in the nucleus

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Atomic Number (Z)

Back 48

The number of protons in the nuclei of any of an element's atoms

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Isotopes

Back 49

Have atoms with the same number of protons but different numbers of neutrons

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Mass Number (A)

Back 50

The numerical sum of the protons and neutrons in the atom

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Periods

Back 51

The rows on the Periodic Table of Elements

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Groups

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The columns on the Periodic Table of Elements

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Representative Elements (Main Group Elements)

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Groups 1, 2, 13, 14, 15, 16, 17, and 18

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Transition Elements

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Groups 3-12

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Inner Transition Elements

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The two rows beneath the table (lanthanides and actinides)

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Lanthanides (Rare Earth Elements)

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Elements 58-71

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Actinides

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Elements 90-103

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Alkali Metals

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Group 1

Front 59

Alkaline Earth Metals

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Group 2

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Noble Gases

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Group 18; used to be called the inert gases

Front 61

Halogens

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Group 17

Front 62

Metalloids

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B, Si, Ge, As, Sb, Te, Po, At
Have properties of both metals and nonmetals

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Nonmetals

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He, Ne, Ar, Kr, Xe, Rn, Uuo, F, Cl, Br, I, O, S, Se, N, P, C, H

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Metals

Back 64

Everything except what I listed under the metalloids and nonmetals

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Metals- Properties

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Metallic luster (shiny)
Conduct electricity
Conduct heat
Malleability
Ductility
Hardness
Solids at room temperature (except mercury)

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Malleability

Back 66

The ability to be hammerd or rolled into thin sheets

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Ductility

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The ability to be drawn into wire

Front 68

Nonmetals- Properties

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Many are solids at room temperature; some are gases
Don't conduct heat or electricity
Not malleable or ductile

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Metalloids- Properties

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Semiconductors
Usually behave as nonmetals

Front 70

Chemical Formulas

Back 70

When chemical symbols are used to represent atoms of the elements that are present

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Free Elements

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One that is not combined with another element in a compund\

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Diatomic molecules

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Molecules composed of two atoms each

Front 73

Hydrates

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Compounds whose crystals contain water molecules in fixed ratios

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Molecule

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An electrically neutral particle consisting of two of more atoms; this term can also be applied to elements such as diatomic hydrogen or oxygen, or molecular compounds

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Chemical Bonds

Back 75

Electrical attractions which hold molecules together

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Molecular formulas

Back 76

Specify the actual numbers of atoms of each kind that make up a single molecule

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Hydrides

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Compounds that elements form with hydrogen

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Organic Compounds

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Compounds that contain carbon; constitute organic chemistry

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Hydrocarbons

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Compounds of carbon and hydrogen

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Alkane Series

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The first six members of the series of hyrdocarbons, including methane, ethane, propane, butane, pentane, and hexane

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Alcohols

Back 81

The atoms OH replace a hydrogen in the hydrocarbon

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Ions

Back 82

When there are more/less electrons than in the normal state of the atom

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Ionic Compound

Back 83

Formed when metal react with nonmetals; when atoms are lost or gained between atoms

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Cation

Back 84

A positively charged ion

Front 85

Anion

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A negatively charged ion

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Transition Metals

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Cr, Mn, Fe, Co, Ni, Cu, Zn, Ag, Cd, Au, Hg

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Post-transition Metals

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Occur right after the transition metals; Sn, Pb, Bi

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Binary Compound

Back 88

Compounds formed from two different elements

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Polyatomic ion

Back 89

Ions that are themselves composed of two or more atoms linked by the same kinds of bonds that hold molecules together

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Nomenclature

Back 90

The naming of molecular and ionic compounds

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Monatomic

Back 91

One atom

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Limiting Reactant

Back 92

Limits the amount of product that forms

Front 93

Excess Reactant

Back 93

Have more of it than is need to completely consume all the other element/compound