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Chem 1410 > Chemestry > Flashcards

Chemestry Flashcards

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1
Q

Pauli Exclusion Principle

A

No 2 electrons can have the same set of 4 quantum numbers.

Atomic orbital can hold 2 electrons and they must have opposing spins.

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2
Q

Aufbau principle

A

“Build up” the lowest energy orbitals are filled first

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3
Q

Hund’s Rule

A

When orbitals of equal energy are available the electron configuration of lowest energy has the maximum number of unpaired

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4
Q

Ionic

A

Metal and nonmetal or metal together

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5
Q

Covalent

A

Two non-metals

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6
Q

Binary molecular compounds

A

Contain atoms of two different nonmetals

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7
Q

Speed of light in a vacuum

A

c = 2.998 x 10^8 m/s

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8
Q

Planck’s constant

A

h = 6.626 x 10^-34 j*s

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9
Q

Avogadro’s constant

A

NA = 6.022 x 10^23

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10
Q

Seven element occur as diatomic molecules (molecules consisting of 2 atoms)

A 
Br
Cl
F
H
I
N
O
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11
Q

In a covalent compound name, you must specify the number of atoms of each element

A

However, if The prefix on the fist atom is mono-, it is not included in the name. Ie. CO2 is carbon dioxide not monocarbon dioxide

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12
Q

Oxidizing agent

A

Species that gets reduced
Gain of electrons
Decrease in oxidation state

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13
Q

Reducing agent

A

Species that gets oxidized
Loss of electrons
Increase in oxidation state

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14
Q

Diatomic elements

A

H2, N2, O2, F2, Cl2, Br2, I2

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15
Q

Reducing agent

A

LEO: Loses Electrons Oxidized

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16
Q

Oxidizing agent

A

GER: Gain Electrons Reduced

17
Q

Combustion analysis

A

Laboratory technique to help determine empirical formula of chemical compound that contain C & H

18
Q

Synthesis reaction

A

Simple substances combine to form more complex substances

A+B—->AB

19
Q

Decomposition reaction

A

More complex substances break down into simpler ones

AB—>A+B

20
Q

Single-replacement reaction

A

An element displaced another element within a compound

A+BC—>AC+B

21
Q

Double-replacement reaction

A

Ionic compounds exchange anions

AB+CD—>AD+CB

22
Q

Combustion reaction

A

A substance, often referred to as fuel, rapidly combines w/oxygen, generally producing carbon dioxide and water

CxHy+O2—>CO2+H2O

23
Q

Enthalpy

A

Combination of changed in heat energy

24
Q

Entropy

A

Randomness

25
Q

Precipitation reaction

A

Double-replacement reaction that results in formation of a lower energy solid ionic compound (produces a precipitate)

*formation of solid

26
Q

Acid-based (neutralization) reaction

A

Reaction of an acid and base with neutralization is its driving force, products are a salt and often water.

27
Q

Oxidation-reduction (redox)

A

Single-replacement, synthesis and decomposition reactions transferring electrons to form lower energy products.

*oxidation is happening

28
Q

Electrolyte

A

Substance that dissolved in water to produce a sol’n that conducts electricity. Aqueous Ionic compounds are known as strong electrolytes because they dissociate 100% to produce sol’ns that conduct electricity readily.

29
Q

Thermochemistry

A

Study of heat and energy in chemical reactions

30
Q

Endothermic reactions

A

Absorb heat from surroundings and have positive deltaH values

31
Q

Exothermic reactions

A

Release heat to surroundings and have negative deltaH values

32
Q

Calorimetry

A

The study of heat transfers by measuring the temperature changes in substances involved

33
Q

Polar bonds

A

Ionic: 2 - 4
Polar covalent: 0.5 - 2
Nonpolar covalent: 0 - 0.5

34
Q

Kinetic energy (energy of motion)

A

KE = 1/2 mv^2

Kinetic energy = 1/2 (mass x velocity)squared

35
Q

Commonly used units for energy

A

1 cal = 4.184 J

calorie & joule

36
Q

Solute

A

Substance(s) dissolved in solvent

37
Q

Solvent

A

The component of the solution that is present in the greatest amount.

38
Q

Light

A

Is a form of energy that is usually thought of as a moving wave of magnetic and electrical potential

39
Q

Visible light

A

is light that can be perceived by the human eye

Chem 1410 (9 decks)

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