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Final Flashcards

1
Q

What is the difference between isotopes and ions?

A

Isotopes have more neutrons changing the atomic mass, and ions have different amounts of electrons changing the charge of an ion.

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2
Q

What is the difference between compounds and molecules?

A

A compound is a substance that has two or more elements, while a molecule is composed of the same elements.

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3
Q

What is a molecular equation?

A

It shows the complete neutral formulas for each compound.

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4
Q

What is a complete ionic equation?

A

It lists all of the ions (precipitate) present in the solution.

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5
Q

What is a spectator ion?

A

reactants that doesn’t participate in the reaction

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6
Q

What is a net ionic equation

A

Only showing the reactants that directly participate in a reaction.

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7
Q

What is an Acid?

A

A substance that produces H+ in aqueous solution

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8
Q

What is an Base?

A

A substance that produces OH- in aqueous solution?

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9
Q

What is an Acid-Base Reaction?

A

An acid reacts with base and the two neutralize each other.

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10
Q

What is oxidation?

A

losing electrons and an increase in oxidation state.

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11
Q

What is Reduction?

A

Gaining electrons and a decrease in oxidation state.

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12
Q

What is endothermic reaction

A

reaction that absorbs energy heat from the surroundings.

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13
Q

What is exothermic reaction?

A

a reaction gives off energy to the surroundings.

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14
Q

Extensive property

A

The amount of matter being heated. It is usually proportional to the amount of reactants that react.

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15
Q

What is delta E

A

The measure of both heat and work exchanged with the surroundings.

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16
Q

What is Delta H

A

The measure of only the heat exchanged under the conditions of constant pressure.

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17
Q

What is a state function?

A

The value depends on the state of the products and the state of the reactants.

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18
Q

Enthalpy of reaction

A

The enthalpy difference between the products and the reactants for chemical reaction.

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19
Q

What is an orbital?

A

It is a probability distribution map of where the electron is likely to be found.

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20
Q

Principal quantum number

A

N it determines the overall size and energy of an orbital.

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21
Q

Angular momentum quantum number

A

L it determines the shape of the orbital.

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22
Q

what shape of the orbital if it the angular momentum quantum number is 2

A

d orbital

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23
Q

what shape of the orbital if it the angular momentum quantum number is 1

A

p orbital

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24
Q

what shape of the orbital if it the angular momentum quantum number is 0

A

s orbital

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25
Magnetic Quantum Number
ml specifies the orientation of the orbital in space.
26
Spin Quantum Number ms
Orientation of the spin of the electron
27
Pauli exclusion Principle
No two electrons in the same atom can have the same set of all four quantum numbers. Orbitals can hold no more than two electrons each. When two electrons occupy the same orbital their spins are opposite.
28
What does shielding do?
it causes the electron to experience a lower positive charge from the nucleus and therefore a higher energy according to coulomb's law.
29
What is penetration?
allows the outer electron to experience a greater nuclear charge and therefore a lower energy.
30
Aufbau Principle
An atom is built up by progressively adding electrons starting from the lowest energy level
31
Hunds rule
When filling up the orbitals that have the same energy the electrons fill them singly first then pair them.
32
the trends for atomic radius
Increases down a column and decreases from left to right. It is almost the same for transitional metals it increases as it goes down but stays roughly the same across the row.
33
ionization energy
the energy required t remove an electron from the atom or ion in the gaseous state
34
Trends ionic radius
ionic radius decreases as it goes from left to right and it increases from top to bottom.
35
trends IE
IE generally increases from left to right. and it decreases from top to bottom
36
trends for metallic character
decreases from left to right and it increases from up to down.
37
exception to octet rule
Molecules or ions with fewer than eight electrons molecules or ions with more than eight electrons around an atom molecules or ions with an odd number of electrons
38
Resonance
depicts two or more structures with electrons in different places to more accurately reflect the delocalization of electrons
39
resonance structure
One of the two or more Lewis structures that have the same skeletal formula but different electron arrangements.
40
resonance hybrid
The actual structure of the molecule is intermediate between two or more resonance structures.
41
electronegativity
the ability of an atom to attract bonding electrons to itself in a chemical bond.
42
polarity
chemical bond depends on the electronegativity difference between two bonding atoms.
43
what type of bond is it if it is smaller than 0.4
pure covalent
44
what type of bond is it if it is bigger than 1.8
ionic
45
if the electronegativity difference is between 0.4 and 1.8
it is a polar covalent bond.
46
How to calculate bond order
#Bonds/ #bond groups
47
VSEPR theory
the electron groups around the central atom repel one another through Coulombic forces.
48
molecular geometry
the geometrical arrangement of atoms in a molecule
49
electron geometry
the geometrical arrangement of electron groups in a molecule
50
polar molecules
the molecules with positive and negative ends
51
nonpolar molecules
the molecules without positive and negative ends
52
when breaking a bond it is
endothermic
53
when a bond forms it is a?
it is exothermic
54
What is the shape of a compound that has 2 electron pairs and has zero lone pairs.
linear and has 180 degree
55
What is the shape of a compound that has 3 electron pairs and zero lone pairs?
trigonal planar and 120 degrees
55
What is the shape of a compound that has 3 electron pairs and one lone pair?
bent or angular and less than 120 degree
56
What is the shape of a compound that has 4 electron pairs and one lone pairs?
Trigonal pyramid and less than 109 degrees.
56
What is the shape of a compound that has 4 electron pairs and zero lone pairs?
Tetrahedral 109 degrees.
57
What is the shape of a compound that has 4 electron pairs and two lone pairs?
bent or angular and less than 109 degrees
58
What is the shape of a compound that has 5 electron pairs and zero lone pairs?
trigonal bipyramid and 90 degrees
59
What is the shape of a compound that has 5 electron pairs and one lone pairs?
sawhorse or seesaw and 90 degrees and 120 degrees
60
What is the shape of a compound that has 5 electron pairs and two lone pairs?
t shape and less than 90 degrees and less than 120 degrees.
61
What is the shape of a compound that has 5 electron pairs and 3 lone pairs?
linear and the degrees is 180
62
What is the shape of a compound that has 6 electron pairs and zero lone pairs?
Octahedral and has 90 degrees
63
What is the shape of a compound that has 6 electron pairs and one lone pairs?
square pyramid and the degrees are less than 90 degrees
64
What is the shape of a compound that has 6 electron pairs and two lone pairs?
square planar and the degree is 90
65
What is the shape of a compound that has 6 electron pairs and three lone pairs?
t shape and less than 90 degrees
66
What is the shape of a compound that has 6 electron pairs and four lone pairs?
linear and less than 180 degrees.

General Chemistry (1 decks)

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