Chapter 1-3 Test Flashcards by Sophia Lim

What is matter?

Anything that occupies space and has mass (forms of energy aren’t matter)

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What is a pure substance?

Uniform chemical composition

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What is a mixture?

Composed of two or more pure substances and may or may not have uniform composition

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Two different types of pure substances

Element and compound

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What is an element?

Cannot be broken down

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Different kinds of elements

Metals, metalloids, nonmetals

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What is a compound?

Composed of 2 or more elements combine in definite proportions

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Metal

Lustrous, malleable, ductile, conductor of heat and electricity, usually solid at room temperature

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Nonmetal

Dull, brittle, insulator of heat and electricity, may be solid, liquid, gas, at room temperature

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Metalloid

Has properties of both metal and nonmetal

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Atom

Smallest unit of an element that retains the chemical properties of that element

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Molecule

Smallest unit of a compound that retains the chemical properties of that compound

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Different types of mixtures

Homogenous and heterogeneous

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Homogeneous

Same composition throughout, dissolved, mixed properly

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Heterogeneous

Don’t have uniform composition (ie potting soil)

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Property

A characteristic that we can observe

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Change

Process that changes the properties of a substance

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Physical property

A characteristic we can observe

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Qualitative physical property

Color, odor

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Quantitative physical property

Mass, density

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Physical change

A process in which no new substances are produced

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Chemical property

A characteristic that can only be observed when a substance is converted

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Density

D = m/v

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Energy

Capacity to do work or transfer heat

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Kinetic energy

Energy of motion

Potential energy

Energy possessed by an object because of its position

Exothermic process

Processes that release energy

Endothermic process

Processes that require energy input

Scientific method

Observation -> Hypothesis -> Experiment -> Conclusion (theory)

Scientific notation

Decimal to the right equals negative exponent, decimal to the left equals positive exponent

Laws of conservation of mass

Mass is not gained or lost in a chemical reaction

Law of definite proportions

A compound always has the same mass ratio of the elements that compose it

Dalton's Atomic theory

All matter is composed of atoms, AL atoms of an element are identical in physical and chemical properties, atoms are not created or destroyed in reactions, atoms rearrange into new combinations, obeying the law of conservation of mass

Temp

Change in heat

Structure of an atom

Composed of subatomic particles and nucleus

Protons

Located in a tiny core at the center of the atom with a positive charge. Can count on right hand corner of element in periodic table

Neutrons

In nucleus, no charge. Can be counted by subtracting proton number from mass number

Electrons

Occupies empty space around nucleus, negative charge. Number is equal to proton number

Atomic number

Number of protons in an atom. Protons + neutrons

Isotope

An atom that contains a specific number of neutrons (will have number of protons from element)

Isotopic symbol

Ions

Differ from atoms in that they have a charge, the number of electrons do not equal protons

Cations

Positively charged ions, fewer electrons

Anions

Negatively charged, more electrons

Group or family

Elements in the same column behave similarly

Period

Horizontal row

Ionic compounds

Made of cation (the metal) and anion (the nonmetals)

Name of cation

Name of metal + "ion"

Roman numerals

Used to indicate the (+). (ie copper 2+ is copper (II) ion)

Cations with predictable charges

Alkali metals (+1), alkaline metals (+2)

Anions

One non-metal, monoatomic group of nonmetals, polyatomic

N -3

Nitride

P -3

Phosphide

O -2

Oxide

S -2

Sulfide

F -1

Fluoride

Cl -1

Chloride

Br -

Bromide

I -

Iodide

Polyatomic ions

Consists of a group of atoms, usually nonmetals

S -2

Sulfide

SO3 -2

Sulfite

SO4 -2

Sulfate

Only common polyatomic cation

NH4 +

CO3 -2

Carbonate

NO2 -

Nitrite

NO3 -

Nitrate

PO3 -3

Phosphite

PO4 -3

Phosphate

SO3 -2

sulfite

SO4 -2

Sulfate

HCO3 -1

Hydrogen carbonate

HPO4 -2

Hydrogen phosphate

H2PO4 -

Dihydrogen phosphate

Halogens have

One negative charge

FO-

Hypofluorite

FO2-

Fluorite

FO3 -

Fluorate

FO4 -

Perfluorate

BrO -

Hypobromite

BrO2 -

Bromite

BrO3 -

Bromate

BrO4 -

Perbromate

MnMPO4

Permanganate ion

CrO4 -2

Chromate ion

OH-

Hydroxide ion

C2H3O2 -

Acetate ion

NH4 +

Ammonium ion

Types of compounds

Metal first = ionic, H first = acid, NO metal at all = molecular

Reactant

A substance that we start with that under goes a change

Product

A new substance that forms during the reaction

Evidence of reaction

Change in color, production of light, formation of solid or gas, change in heat

Chemical equations

Subscript after formulas, (S) (g) (L)

Relative atomic mass

(isotope mass of isotope 1) x (relative abundance of isotope 1) + (isotope mass of isotope 2) x (relative abundance of isotope 2)

Alkali metals

Group 1 metals

Alkaline metals

Group 2 metals

Halogens

Group 17 nonmetals

Noble gases

Group 18 nonmetals

Main-group elements

Contain any element in the 8 groups designated with the letter A, groups 1, 2, and 13-18

Transition metals

Groups 3-12

7 elements that exist as diatomic molecules

N2, O2, F2, C12, Br2, I2, H2

Metals tend to lose electrons

To become cations, to have the same number of electrons as the last noble gas

Nonmetalls tend to gain electrons

To become anions, to have the same number of electrons as the next noble gas

Acids

A substance that loses an H+ when reacting with water

Bases

Substances that losee an OH- when reacting with water

Binary acids

Made from hydrogen + one non-metal. Use hydro prefix and - ic

HF (aq)

Hydrofluoric acid

HCI (aq)

Hydrochloric acid

HI (aq)

Hydroiodic acid

H2S (aq)

Hydrosulfuric acid

Oxyacids

Made from hydrogen and polyatomic anion. - ate becomes - ic, - ite becomes - ous, - ide

Water

H2O

Ammonia

NH3

Methane

CH4

Sodium chloride

NaCl

Sodium nitrite

NaNO2

Magnesium chloride

MgCl2

Magnesium nitrate

Mg(NO3) 2

Barium oxide

BaO

Lithium nitride

Li3N

Chapter 1-3 Test Flashcards

(120 cards)