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289 Cards in this Set

  • Front
  • Back
3) Plan and do additional experiments to test the hypothesis
4) Modify the hypothesis as necessary so that it is compatible wit hall the pertinent data
Scientific Method
Scientific laws
The quantity or amount of matter that an object possesses
A measure of the earth's gravitational attraction for a body
Significant figures
Rounding off numbers
Scientific notation
Metric system or SI
A unit of volume commonly used in chemistry; =1000 mL
The mass of an object divided by its volume
Specific gravity
Anything that has mass and occupies space
Without shape or form
A particular kind of matter with a definite, fixed composition
Uniform in appearance and has the same properties throughout
Matter consisting of two or more physically distinct phases
Simply the body of matter under consideration
Smallest particle of an element
Abbreviation of an element, Ba I N O Ag
A positively or negatively charged atom or group of atoms
Positively charged ions
Negatively charged ion
Diatomic molecules
Chemical formula
Physical properties
Chemical properties
Physical changes
Chemical change
Chemical equations
The starting substances (water, copper, and oxygen)
Law of Conservation of Mass
The capacity of matter to do work
Potential energy (PE)
Energy that matter possesses due to its motion.
Kinetic energy (KE)
The SI unit of energy, see also calorie
Specific heat
Law of Conservation of Energy
Dalton's atomic model
Law of Definite composition
Law of Multiple proportions
Electrons, protons, and neutrons
Subatomic particles
Electron (e-)
Thomson model of the atom
Atomic Number
Atomic Mass Unit
Atomic Mass
The system of names that chemists use to identify compounds
Chemical nomenclature
Compounds that do not generally contain carbon
Inorganic compounds
Diatomic molecules
Most often ions are formed when metals combine with ____________
Compound that contains only two different elements
Binary compound
1) Cu 1+, copper (I)
2) Cu 2+, copper (II)
4) HG 2+, Mercury (II)
1) Cuprous
2) Cupric
3) Mercurous
4) Mercuric
1) Fe 2+, Iron (II)
2) Fe 3+, Iron (III)
3) Sn 2+, Tin (II)
4) Sn 4+, Tin (IV)
5) Pb 2+, Lead (II)
1) Ferrous
2) Ferric
3) Stannous
4) Stannic
5) Plumbous
1) Pb 4+, Lead (IV)
2) As 3+, Arsenic (III)
3) As 5+, Arsenic (V)
4) Ti 3+, Titanium (III)
5) Ti 4+, Titanium (IV)
1) Plumbic
2) Arsenous
3) Arsenic
4) Titanous
5) Titanic
1) Nona
2) Hepta
3) Tetra
4) Mono
1) 9
2) 7
3) 4
5) 1
1) Deca
2) Octa
3) Hexa
4) Penta
5) Tri
6) Di
1) 10
2) 8
3) 6
4) 5
5) 3
6) 2
disulfur decafluoride
carbon tetrachlorid
dinitrogen pentaoxide
Composed of hyrdrogen and one other nonmetallic element
Binary acids
Binary Acids
1) HF
2) HCl
3) H₂S
1) Hydrofluoric acid
2) Hydrochloric acid
3) Hydrosulfuric acid
1) HBr
2) HI
3) H₂Se
1) Hydrobromic acid
2) Hydroiodic acid
3) Hydroselenic acid
2) Write the word acid
Naming binary acids
An ion that contains two or more elements
Polyatomic ion
1) Acetate
2) Ammonium
3) Arsenate
4) Hydrogen carbonate
5) Hydrogen sulfate
6) Bromate
7) Carbonate
8) Chlorate
9) Chromate
1) C₂H₃O₂⁻
2) NH₄⁺
3) AsO₄ 3-
4) HCO₃⁻
5) HSO₄⁻
6) BrO₃⁻
7) CO₃ 2-
8) ClO₃⁻
9) CrO₄ 2-
1) Cyanide
2) Dichromate
3) Hydroxide
4) Nitrate
5) Nitrite
6) Permangante
7) Phosphate
8) Sulfate
9) Sulfite
1) CN⁻
2) Cr₂O₇ 2-
3) OH⁻
4) NO₃⁻
5) NO₂⁻
6) MnO₄⁻
7) PO₄ 3-
8) SO₄ 2-
9) SO₃ 2-
Stock System
1) Hypochlorite
2) Chlorite
3) Chlorate
4) Perchlorate
1) ClO⁻
2) ClO₂⁻
3) ClO₃⁻
4) ClO₄⁻
1) Hypochlorous acid
2) Chlorous acid
3) Chloric acid
4) Perchloric acid
1) HClO
2) HClO₂
3) HClO₃
4) HClO₄
1) Sulfate ion
2) Sulfite ion
3) Nitrate ion
4) Nitrite ion
5) Carbonate ion
6) Borate ion
1) SO₄ 2-
2) SO₃ 2-
3) NO₃⁻
4) NO₂⁻
5) CO₃ 2-
6) BO₃ 3-
1) Phosphate ion
2) Phosphite ion
3) Iodate ion
4) Acetate ion
5) Oxalate ion
6) Bromate ion
1) PO₄ 3-
2) PO₃ 3-
3) IO₃⁻
4) C₂H₃O₂⁻
5) C₂O₄ 2-
6) BrO₃⁻
1 mol, 6.022 x 10^23
Avagadro's Number
6.022 x 10^23 items=
1 mole
The mass of avogadro's number of atoms or molecules

Molar Mass
The mass percent represented by each element in a compound
Percent composition of a compound
Empirical formula
Molecular formula
The substances entering the reaction are called
the reactants
The substances formed are called
the products
Chemical equation
Balanced equation
Combination reaction

A + BC ---- B + AC or
A + BC ---- C + BA
Single-displacement reaction

AB --- A + B
Decomposition reaction
Two compounds exchange partners with each other to produce two different compounds

AB + CD ---- AD + CB
Double-displacement reaction
Liberate heat
Exothermic reactions
Absorb heat
Endothermic reactions
The quantity of heat produced by a reaction is known as
Heat of reaction
Compounds containing only hydrogen and carbon
Activation energy
Molar mass
Relationship between molecule and mole
Mole ratio
It limits the amount of product that can be formed
Limiting reactant
Theoretical yield
The amount of product that we finally obtain
Actual yield
Percent yeild
The distance between consecutive peaks (or troughs) in a wave
Tells how many waves pass a particular point per second
Tells how fast a wave moves through space
Line spectrum
Ground state
Principal energy levels of electrons
Each principal energy level is divided into
Pauli exclusion principle
The orbital arrangement of electrons in an atom
Electron configuration
Valence electrons
Each horizontal row in the periodic table is called a
Groups or Families
The A groups are known as the
Representative elements
The B groups and Group VIII are called
Transition elements
Ionization energy
Lewis structure
The attraction between oppositely charged ions
Ionic bond
Consists of a pair of electrons shared between two atoms
Covalent bond
Polar covalent bond
Nonpolar covalent
Linear structure
trigonal planar structure
tetrahedral structure
Kinetic-molecular theory (KMT)
Ideal Gas
KE (Kinetic Energy)
Graham's law of effusion
Defined as forcer per unit area
Atmospheric Pressure (ATM)
A device used to measure atmospheric pressure
1 atmosphere (atm)

P₁V₁ = P₂V₂
Boyle's law
Absolute Zero

V₁/T₁ = V₂/T₂
Charle's Law

P₁/T₁ = P₂/T₂
Gay-Lussac's Law
Standard Conditions
Standard Temperature and Pressure (STP)
Dalton's law of partial pressures
The pressure exerted independently by each gas in a mixture of gases
Partial pressure
Gay-Lussac's law of combining volumes
Avagadro's law
Molar volume (of a gas)
Mass/Volume or g/L
PV = nRT
Ideal Gas Equation
Solid -------> Vapor
Vapor pressure
Surface tension
Capillary action
Boiling point
Normal boiling point
Vapor-pressure curve
Freezing or Meling point
Heat of Fusion
Heat of Vaporization
Linear structure
Hydrogen bond
Water in a hydrate is known as
Water of hydration
Water of crystallization
"without water"
The dissolving agent or the most abundant component in a solution
Liquids that are capable of mixing and forming a solution
Concentration of a solution
A solution containing dissolved solute in equilibrium with undissolved solute
Saturated solution
Unsaturated solution
Supersaturated solution
Describes a solution that contains a relatively small amount of dissolved solute
Dilute solution
Contains a relatively large amount of dissolved solute
Concentrated solution
g solute/g solute + g solvent X 1,000,000 =
Parts per million (ppm)
g solute/ g solute + g solvent X 100 =
Mass percent
number of moles of solute
_________________________ =

liter of solution
Molarity (M)
Colligative properties
Semipermeable membrane
A solution contains an excess of H⁺ ions
Arrhenius acid
A solution contains an excess of OH⁻ ions
Arrhenis base
A acid is a proton (H⁺) donor
Bronsted-Lowry acid
A base is a proton (H⁺) acceptor
Bronsted-Lowry base
Hydronium ion
An electron-pair acceptor
Lewis acid
An electron-pair donor
Lewis base
A substance having properties of both an acid and a base
Substances whose aqueous solutions are conductors of electricity are called
Substances whose solutions are nonconductors are known as
Acids, bases, and salts are __________
Are essentially 100% ionized in solution
Strong electrolytes
Are much less ionized (based on comparing 0.1 M solutions)
Weak electrolytes
-log[H⁺] =
pH < 7.00
Acidic solution
pH = 7.00
Neutral solution
pH > 7.00
Basic solution
The power to which 10 must be raised to give that number
Spectator ions
Compounds are written in their molecular, or formula expressions
Un-ionized equation
Total ionic equation
Only those molecules or ions that have changed are included in the equation; ions are molecules that do not change (the spectators) are omitted
Net ionic equation
A dispersion in which the dispersed particles are larger than the solute ions or molecules of a true solution and smaller than the particles of a mechanical suspension
The random motion of colloidal particles are called
Brownian movement
An intense beam of light is clearly visible when passed thourhg a colloidal dispersion, but is not visible when passed through a true solution
Tyndall effect
Dissovled solutes can be removed from colloidal dispersions through the use of such a membrane by a process called _____.
The process by which a parchment membrane allows the passage of true solutions, but prevents passage of colloidal dispersions
The total mass remains constant during a chemical reaction. What law is this?
Law of conservation of mass
All samples of a compound have the same composition; that is, all samples have the same proportions, by mass, of the elements present in the compound. What law is this?
Law of constant composition
In two or more compounds of the same elements, the masses of one element that comine with a fixed mass of the second element are in the ratio of small whole number. What law is this?
Law of multiple proportions
What has a relative mass of 1, also carries one fundamental unit of positive electric charge, denoted 1+?
What is an electrically neutral particle; it has no charge, has a slightly greater mass than that of the proton?
What has a mass that is 1/1836 of the mass of a proton, has the same quantity of charge as a proton, but it is a negative charge, denoted as 1-?
Protons and neutrons are densely packed into a tiny, positively charged core of atom known as the _________.
What is the number of protons in the nucleus of an atom of a give element?
Atomic number (Z)
Atoms that have the same number of protons but different numbers of neutrons are called _______.
What is the sum of the numbers of protons and neutrons in an atom, always an integral (whole) number.
Mass number (A)
Exactly one-twelth the mass of a carbon-12 atom
Atomic Mass Unit
1.66054 X 10^-24 g =
1 amu or u
What is the weighted average of the masses of the naturally occurring isotopes of that element?
Atomic mass
Mendeleev arranged the elements in order of increasing atomic weight, from left to right in rows and from top to bottom in columns (or groups). Elements that most closely resemble one another in physical and chemical properties tend to fall in the same vertical group. This group similarity recurs periodcially, hence the name __________ ________.
Periodic Table
Elements that lack metalic properties, to the right of the stepped line are ________
Some of the elements bordering the stepped line resemble metals in some of their properties and nonmetals in other. They are sometimes considered in a special category called semimetals or _________
A symbolic representation of the composition of a compound expressed in terms of its constituent elements is a ____________ _________
Chemical formula
A group of two or more atoms held together in a definite spatial arrangement by forces called covalent bonds
Molecules are the smallest characteristic entites of a ______ ________, and these molecules determine the properties of the substance.
Molecular compound
The simplest formula we can write for a compound. It lists the elements present and indicates the smallest integral (whole-number) ratio in which atoms of these elements are combined
Emperical formula
Show the differences between compounds with identical empirical formulas by giving the symbol and the actual number of each kind of atom in a molecule
Molecular formula
A chemical formula that shows how atoms are attached to one another
Structural formula
A individual atom or a group of bonded atoms may lose or gain one ore more electrons, thereby acquiring a net electric charge and becoming and _______
Positively charged ions are called _______
Negatively charged ions are called ________
Oppositely charged ions (cations and anions) attract one another and are held together in huge clusters by electrostatic attractions, such clusters are called _________ _________
Ionic compounds
Because ionic compounds do not consist of discrete molecules, we base the chemical formula on the simplest collection of cations and anions that represents an electrically neutral unit. We call this hypothetical collection of ions a _______ ______ of the compound.
Formula unit
A charged group of bonded atoms--for example, NH₄+ or SO₄2-
Polyatomic ion
A ionic compound in which the formula unit includes a fixed number of water molecules associated with the cations and anions
Substances that have the following characteristics when dissolved in water:
- Tasts sour if diluted with enough water to be tasted safely
- Produce a pricking or stinging sensation on the skin
- Turn the color of litmus, an indicator dye, from blue to red
- React with many metals to produce ionic compounds and hydrogen gas
- React with bases, thereby losing their acidic properties
Are substances that have the following characteristics when dissolved in water:
- Taste bitter if diluted with enough water to be tasted safely
- Feel slippery or soapy on the skin
- Turn the color of the indicator dye litmus from red to blue
- React with acids, thereby losing their basic properties
A molecular compound (such as HBr) that ionizes, or breaks up, in water to form a solution containing H+ cations plus anions (such as Br-)
Arrhenius acid
A compound that ionizes in water to form a solution containing OH- anions and related cations
Arrhenius base
The cation from the base and the anion from the acid make up an ionic compound called a _______