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Chem Final (Miscellaneous 1-9)
N/A
126
Chemistry
11th Grade
01/12/2010

Additional Chemistry Flashcards

 


 

Cards

Term
What is chemistry?
Definition

EveryTHING

All matter

Term
When are we the "smartest"?
Definition
As babies. We test everything.
Term
What are the 3 steps of the scientific method?
Definition
Observation, Hypothesis, Experimentation
Term
What is a law?
Definition
A summary of observed behavior.
Term
What is a theory?
Definition
An explanation of behavior.
Term
A measurement must always consist of a _____ and a _____.
Definition
number, unit
Term
125 = ?
Definition
125 = 1.25 x 102
Term
1700 = ?
Definition
1.7 x 103
Term
93,000,000 = ?
Definition
9.3 x 107
Term
0.010 = ?
Definition
1.0 x 10-2
Term
0.000167 = ?
Definition
1.67 x 10-4
Term
What are the two most widely used systems?
Definition
English system, Metric system
Term
What is the fundamental SI (International System) unit for mass?
Definition
Kilogram (kg)
Term
What is the SI unit of length?
Definition
Meter (m)
Term
What is the fundamental SI unit for time?
Definition
second (s)
Term
What is the fundamental SI unit for temperature?
Definition
Kelvin (K)
Term
What is the prefix for 1,000,000?
Definition
mega (M)
Term
What is the prefix for 1000?
Definition
Kilo (k)
Term
What is the prefix for 0.1?
Definition
Deci (d)
Term
What is the prefix for 0.01?
Definition
Centi (c)
Term
What is the prefix for 0.001?
Definition
Milli (m)
Term
What is the prefix for 0.000001?
Definition
Micro (µ)
Term
What is the prefix for 0.000000001?
Definition
Nano (n)
Term
1 meter = ______ inches
Definition
39.37
Term
what is the unit for 1000 m?
Definition
Kilometer (km)
Term
what is the unit for 0.1 m?
Definition
Decimeter (dm)
Term
What is the unit for 0.01 m?
Definition
Centimeter (cm)
Term
What is the unit for 0.001 m?
Definition
Millimeter (mm)
Term
What is the unit for 0.000001 m?
Definition
Micrometer (µm)
Term
What is the unit for 0.000000001 m?
Definition
Nanometer (nm)
Term
1 inch = _____ cm
Definition
2.54
Term
Volume = ?
Definition
1m x 1m x 1m = 1m3
Term
1 Liter (L) = _____ mL
Definition
1000
Term
1 kg = _____ g
Definition
1000
Term
1 g = _____ mg
Definition
1000
Term

When rounding, round to the 1st uncertain digit.

 

 

Definition
9.874312 cm = 9.87 cm
Term
When do nonzero integers count as SigFigs?
Definition
Always.
Term
When do leading zeros count as SigFigs?
Definition

Never.

Ex. 0.00067

Term
When do captive zeros count as SigFigs?
Definition

Always.

Ex. 0.67089

Term
When do trailing zeros count as SigFigs?
Definition

Only when there is a decimal point.

 

896000 not SigFigs

896000. SigFigs

Term
Explain "exact numbers".
Definition

Discovered by counting. Can be assumed to have an unlimited number of SigFigs.

 

Ex. 1 in = 2.54 cm

Neither 2.54 nor 1 limits the amount of SigFigs when used in a calculation.

Term
Rounding for multiplication and division.
Definition

Ex. 4.56 x 1.4 = 6.384 = 6.4

 

Ex. 8.315 ÷ 298 = 0.0279027 = 2.79 x 10-2

Term
Rounding for adding and subtraction.
Definition

Ex. 12.11 + 18.0 + 1.013 = 31.123 = 31.1

 

Ex. 0.6875 - 0.1 = 0.5875 = 0.6

Term
Define conversion factor.
Definition
A ratio of the two parts of the statement that relates the two units. 
Term
Conversion Factor
Definition

Ex. 2 dozen doughnuts x 12 ÷ 1 dozen = 24 doughnuts

 

Dozens cancel out.

Term
Equivalence statement.
Definition
Ex. 2.54 cm = 1 inch
Term
Equivalence statement 2.54 cm = 1 inch leads to what conversion factors?
Definition

2.54 cm ÷ 1 inch 

or

1 inch ÷ 2.54 cm

Term
Converting Celsius to Kalvin.
Definition

C + 273 = K

 

K- 273 = C

Term
Density.
Definition
Density = mass ÷ volume
Term
Mass.
Definition
Volume x density = mass
Term
Volume. 
Definition
Volume = mass ÷ density
Term
What are the 3 things scientists look at when observing matter?
Definition
Composition, structure, and behavior.
Term
What are the 3 forms of matter?
Definition
Solid, liquid, gas.
Term
Define solid.
Definition
Rigid; has a fixed shape and volume.
Term
Define liquid.
Definition
Has a definite volume, but takes the shape of its container.
Term
Define gas.
Definition
Has no fixed volume or shape; takes the shape and volume of its container. 
Term
List some physical properties. 
Definition
Odor, color, volume, state, density, melting point, and boiling point. 
Term
List some chemical properties.
Definition
Wood burning, giving off heat, rusting of steel. 
Term
List some physical changes. 
Definition
Ice to water to water vapor.
Term
List some chemical changes.
Definition
A change in the composition of the substance; reactions. 
Term
What are the 3 ways to separate elements?
Definition
Chromotography, distillation, filtration.
Term
Define element. 
Definition
A substance that cannot be broken down into other substances by chemical methods. 
Term
Define compound. 
Definition
A substance composed of a given combination of elements that can be broken down into those elements by chemical methods.
Term
Define mixture.
Definition

Something that has variable composition. 

Ex. Wood

Term
Define pure substance.
Definition
Something that will always have the same composition.
Term
Define solution.
Definition
A homogeneous mixture.
Term
Define homogeneous.
Definition
The same throughout.
Term
Define heterogeneous.
Definition
Variable composition.
Term
Define distillation.
Definition
The process of boiling a mixture and condensing the water vapor in a separate container, leaving the solids in the 1st container.
Term
Define filtration. 
Definition
Pouring a solution through a mesh, allowing liquids to pass through while solids stay behind.
Term
What is Robert Boyle known for?
Definition
His experimentation and pioneering on the properties of the gases.
Term

What was John Dalton known for?

 

Definition
Dalton's atomic theory.
Term
What are the 5 points of Dalton's atomic theory?
Definition

1. Elements are made of tiny particles called atoms.

2. All atoms of a given element are identical.

3. The atoms of a given element are different from those of any other element.

4. Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers and types of atoms.

5. Atoms are indivisible in chemical process.

Term

Define the law of constant composition. 

 

Definition
A given compound always has the same composition, regardless of where it comes from.
Term
Define compound.
Definition
A distinct substance that is composed of the atoms of two or more elements and always contains exactly the same relative masses of those elements.
Term
What is J.J. Thomson known for?
Definition
The Plum Pudding Model.
Term
What is Rutherford known for?
Definition
The gold foil experiment that reflected particles.
Term
Define Atomic Number.
Definition
The number of protons.
Term
Define Mass Number.
Definition
The sum of protons and neutrons.
Term
Define isotope.
Definition
Atoms with the same number of protons but different numbers of neutrons. 
Term
What is Mendeleev known for?
Definition
Arranging the elements in order of increasing atomic mass.
Term
List physical properties of metals.
Definition

1. Efficient conduction of heat and electricity.

2. Malleability.

3. Ductility.

4. A lustrous appearance.

Term
The elements next to the stair step line in the periodic table are known as?
Definition
Metalloids of semi-metals.
Term
Define diatomic molecules.
Definition
Made up of 2 atoms. (all of the "gens"
Term
Define ion.
Definition
A charged entity.
Term
Define anion.
Definition
Negatively charged ion.
Term
Define cation.
Definition
Positively charged ion.
Term
An ionic compound cannot contain only anions or only cations, because the net charge of a compound must be zero.
Definition
N/A
Term
Define binary compounds.
Definition
Compounds that contain two elements (either a metal and a nonmetal or two nonmetals).
Term
What are the two dependable/non-predictable elements?
Definition
Zinc/Silver
Term
Binary ionic compounds contain on anion and a cation. The cation always comes first.
Definition
N/A
Term

Type 1 compounds- The metal present forms only one type of cation.

Type 2 compounds- the metal present can form two or more cations that have different charges.

Definition
N/A
Term
What is the prefix for 1?
Definition
mono
Term
What is the prefix for 2?
Definition
di
Term
What is the prefix for 3?
Definition
tri
Term
What is the prefix for 4?
Definition
tetra
Term
What is the prefix for 5?
Definition
penta
Term
What is the prefix for 6?
Definition
hexa
Term
What is the prefix for 7?
Definition
hepta
Term
What is the prefix for 8?
Definition
octa
Term
What is the prefix for 9?
Definition
nona
Term
What is the prefix for 10?
Definition
deca
Term
Hydrofluoric acid
Definition
HF
Term
HCl
Definition
Hydrochloric acid
Term
Hydrobromic acid
Definition
HBr
Term
Hydroiodic acid
Definition
HI
Term
Hydrocyanic acid
Definition
HCN
Term
Hydrosulfuric acid
Definition
H2S
Term
Nitric acid
Definition
HNO3
Term
Nitrous acid
Definition
HNO2
Term
Sulfuric acid
Definition
H2SO4
Term
Sulfurous acid
Definition
H2SO3
Term
Phosphoric acid
Definition
H3PO4
Term
Acetic acid
Definition
H2S
Term
Precipitation reaction
Definition
a solid forms (called precipitate)
Term
What is the difference between a molecular equation and a complete ionic equation?
Definition

Ex. Molecular: K2CrO4(aq) + Ba(NO3)2(aq) → BaCrO4(s) + 2KNO3(aq)

 

Ex. Complete Ionic equation

2K+(aq) + CrO42-(aq) + Ba2+(aq) + 2NO3-(aq) → BaCrO4(s) + 2K+(aq) + 2NO3-(aq)

Term
Spectator ions
Definition

Ex. Complete Ionic equation

2K+(aq) + CrO42-(aq) + Ba2+(aq) + 2NO3-(aq) →BaCrO4(s) + 2K+(aq) + 2NO3-(aq)

Term
Net ionic equation
Definition
only contains those that undergo a change. 
Term
Acid-base reaction
Definition

Water is formed when mixed with a strong acid and a strong base.

 

Ex. HCl(aq) + KOH(aq) → H2O(l) + KCl(aq

Acid

Term
Oxidation-reduction reaction.
Definition

Involves a transfer of electrons. 

 

Ex. 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s)

Term
Double displacement reactions.
Definition

AB + CD → AD + CB

 

Ex. K2CrO4(aq) + Ba(NO3)2(aq) → BaCrO4(s) + 2KNO3(aq)

Term
Synthesis reaction
Definition
Ex. 2H2(g) + O2(g) → 2H2O(l)
Term
Decomposition reaction
Definition
Ex. 2H2O(l) → 2H2(g) + O2(g)
Term
Avogadro's number
Definition

6.022 x 1023

 

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