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Chemistry Final Test > Final Test > Flashcards

Final Test Flashcards

(53 cards)

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1
Q

Ion

A

A charged atom

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2
Q

Cation

A

A positive ion

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3
Q

Anion

A

A negative ion

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4
Q

Salt

A

An ionic compound that forms when a metal atom or a positive radical replaces the hydrogen of an acid

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5
Q

Lattice energy

A

The energy associated with constructing a crystal lattice relative to the energy of all constituent atoms separated by infinite distances

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6
Q

Binary compounds

A

The names given to the compounds which contain EXACTLY two elements

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7
Q

Crystal lattice

A

The name given to the regular pattern in which a crystal is arranged

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8
Q

Unit cell

A

The smallest portion of a crystal lattice that shows the 3D pattern of the entire lattice

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9
Q

Ionic bonds

A

Transferring valence electrons between atoms

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10
Q

Covalent bond

A

The sharing of valence electrons between atoms

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11
Q

Ternary compounds

A

Compounds that have EXACTLY three elements

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12
Q

Mole

A

The SI unit of quantity

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13
Q

Avogadro’s number

A

6.02 x 10^23 (602 sextillion)

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14
Q

Molar mass

A

The mass of 1 mile of a given compound or given element

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15
Q

Average atomic mass

A

The weighted average of masses o all isotopes of a given element

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16
Q

Atomic mass unit

A

The unit that is defined to be 1/12 the mass of a carbon-12 atom

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17
Q

Percentage composition

A

Shows the percentage by weight of all elements in a given compound

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18
Q

Empirical formula

A

The simplest whole number ratio of the number of elements in a given compound

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19
Q

Molecular formula

A

The true chemical formula of a given compound

Produced when you simplify q molecular formula

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20
Q

Hydrate

A

A compound which has loosely attached water molecules

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21
Q

Chemical reaction

A

The process in which one or more substances change to produce one or more different substances

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22
Q

Chemical equation

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A

A written representation of a chemical change hitch involves chemical symbols, chemical formulas, an an arrow

23
Q

Reactants

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A

The substances that are present before a chemical change occurs

24
Q

Products

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A

The substances that are produced as a result o a chemical change

25
Law of conservation of matter
"Matter cannot be created nor destroyed but can change form through ordinary chemical reactions" -created by Antoine Lavoisier (French, guillotine)
26
Conversion factor
A fraction that is equivalent to 1, that is used to convert a given unit to a different unit
27
Coefficient
The number placed in front of the molecules represented in an equation to indicate the numerical ratio of the substances reacting
28
Subscript
Small numbers that indicate the number of a particular type of atom or ion in a formula unit
29
Synthesis
Reaction in which two or more substances combine to form one new substance
30
Decomposition
Reaction which one substance breaks down to form two or more new substances
31
Single displacement
A chemical reaction in which an element traded places with an element in a compound
32
Double displacement
A chemical reaction in which an element from a compound trades places with an element from a compound
33
Stoic homered
The quantitative study of chemical reactions
34
Limiting reactant
The substance that is completely used up in a chemical reaction
35
Excess reactant
The substance that still remains, I reacted, when the chemical reaction stops
36
Mass to mass problems
Given a specific amount of mass of a reactant, determine how many grams of reactant can be produced
37
Mass to volume problems
When a chemical reaction occurs and gases are produced, rather than determining the mass of the gas produced, it may be more understandable to determine the "volume" of gas produced
38
STP
Standard pressure and temperature - temperature of 0 degree Celsius at sea level - pressure is 101.3 kilo pascals
39
Molar volume
The volume that one mole of gas particles occupy at STP
40
Avogadro's hypothesis
Equal volume of gases under identical conditions o temperature and pressure, contain the same number of molecules
41
Pressure
The amount of force exerted per unit area of surface
42
Newton
The SI unit of force | -the force that gives an acceleration of 1 m/sec squared to an object whose mass is 1 kg
43
Pascal
The SI u it of pressure | -equal to the force of 1 N exerted over an area of 1 m squared
44
Boyle's Law
For a fixed amount of gas at a constant temperature, the volume of the gas increases as the pressure of the gas decreases an the volume of the gas decreases as the pressure of the gas increases
45
Charle's Law
For a fixed amount of gas at a constant pressure, the volume of a gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases
46
Ideal gas
A fictional, theoretical gas that closely mimics the behavior of real gases -they expand when heated, contract when cooled, but they never condense and they never solidify
47
Ideal gas law
Te mathematical relationship o pressure, volume, temperature, the gas constant K, and the number of miles of a gas n
48
Real gas
An actual gas that expanses when heated, contracts when cooled, eventually condenses and eventually turns into a solid
49
Diffusion
Te movement of particles from regions of higher density to regions of lower density
50
Effusion
The passage of gas under pressure through a tiny opening
51
Graham's Law of diffusion
The rate of diffusion o a gas is inversely proportional to the square root of the gas's density
52
Gay-Lussac's Law of Combining volumes
The law that states that the volume of gases involves Ina chemical change can be represented by the ratio of small whole numbers
53
Valence electrons
Electrons in the outermost energy level which take part in chemical reactions

Chemistry Final Test (1 decks)

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