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AP Chem > Chapter 7 > Flashcards

Chapter 7 Flashcards

0
Q

Heating and purifying a liquid

A

Distillation

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1
Q

Taking out by force using different polarities

A

Extraction

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2
Q

Purifying solids by using differences on solubility

A

Recrystallization

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3
Q

Separates colored pigments developed by Mikhail Tsvet

A

Chromatography

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4
Q

Amount of positive charge from the nucleus that has an effect on the selected electron

A

Effective nuclear charge

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5
Q

Strength of the interaction between two electrical charges depends on the magnitude and distance of the charges

A

Coulomb’s law of attraction

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6
Q

What doesn’t account for repulsion?

A

Finding the attraction between electron and nucleus

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7
Q

What does account repulsion?

A

Effective nuclear charge

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8
Q

Z(eff)= Z - S

A 
Z(eff) = effective nuclear charge
Z= atomic number
S= # of shielding electrons
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9
Q

What is shielding?

A

Electrons closer to the nucleus prevent some of the positive charge from reaching the outer valence electrons (electrons in the same subshell do shielding)

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10
Q

Slaters rules

A

Electrons in the same energy level count as .35 (do not count selected electron)
Electrons in one energy level lower count as .85
All other electrons count as 1.0

S= (x * .35) + (y * .85) + (z * 1.0)

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11
Q

Effective nuclear charge trends

A

Increases across a period

Increases slightly down a group

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12
Q

The sizes of atoms and ions…

A

Do not have defined boundaries

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13
Q

Van der waals

A

Measure distance between two colliding nuclei and divide by two

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14
Q

Bonding atomic radius

A

Divide distance between nuclei by two

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15
Q

Sizes of atoms trends

A

Increases going down a column

Decreases going across a period

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16
Q

What does ionic radii depend on

A

Depends on nuclear charge, number of electrons and the orbital valence electrons reside in

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17
Q

Cations are _____ than parent atoms

A

Smaller because electrons are removed farthest from the nucleus and electron- electron repulsion is reduced

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18
Q

Anions are ______ than parent atoms

A

Bigger

Electron-electron repulsion is increased

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19
Q

Isoelectonic series

A

Group of ions all containing the same number of electrons

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20
Q

Ionization energy

A

Minimum energy required to remove an electron from an isolated gaseous atom or ion so that the electron and resulting ion are a finite distance apart

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21
Q

First ionization energy

A

Energy needed to remove the first electron from a neutral atom

22
Q

Second ionization energy

A

Energy needed to remove the second electron

23
Q

Trends for ionization energy

A

Decreases down groups

Increases across periods

24
Electron affinity
The change in energy of kJ per mole in a neutral atom while an electron is added to make a negative ion
25
Why does oxygen require energy to add 2nd electron?
Electrons out number protons, the nucleus does not attract electrons as strongly and the electrons repel eachother
26
Electron affinity trends
Increases across a period | Decreases down a group
27
Exceptions to electron affinity rules
Noble gases, group 5 metals and group 2 metals require energy to add an electron because they're already stable
28
Metallic character
How closely relatable the element is to the standard properties of a metal
29
Metallic character trends
Decreases across a period | Increases down a group
30
Nonmetallic character
How closely relatable the element is to the standard properties of a nonmetal
31
Metal characteristics
``` Luster, Solid Malleable and ductile Good conductors Form positive ions Ionic bonding ```
32
Nonmetal characteristics
``` No luster Generally gases Brittle Poor conductors Covalent bonds Negative ions ```
33
Metalloids
Elements that have both metal and nonmetal properties
34
Alkali metal characteristics
``` Silver luster Behaves as metals High conductivities Low melting and boiling points Reactive (active metals Exothermic Colorless until set on fire ```
35
Water as a reactive ion (alkali metals)
Forms hydrogen gas and alkali metal hydroxides Exothermic reactions Violent reactions with heavy metals
36
Oxygen ion as a reactive ion (alkali metals)
Complex reactions Lithium forms oxides Sodium forms peroxides Potassium, rubidium and cesium form superoxides
37
Alkali metal trends (down group)
Melting point decreases Densities increase Become softer Reactivity increases
38
Alkaline earth metal characteristics
``` Solids Metallic properties Melt at higher temperatures Hard and sense Less reactive than 1A Change colors when heated by fire Ca: red Ba: green Sr: bright red Ba: green ```
39
Alkaline earth metal trends going down a group
Ease of losing electrons increases | Reactivity increases
40
Water as a reactive ion (alkaline earth)
Mg reacts with steam Na and K react with water Ca reacts with hot water Forms hydrogen gas and hydroxide
41
Nonmetals as reactive ions (alkaline earth)
Loses two electrons in a sublevel Magnesium is least reactive Heavier= more reactive
42
Hydrogen characteristics
Colorless, odorless, lowest density | More than double ionization energy compared to other metals, properties of metal and nonmetal
43
Oxygen group (chalcogens) trends
Melting point, boiling point, ionization energy, electro negativity, density, atomic radius, toxicity and ionic radius increase as you go down
44
Halogens characteristics
Poor conductors, low melting and boiling points, forms ionic salts, highly reactive, decrease down a group, easily dissociate
45
Noble gases characteristics
Colorless, monoatomic, large ionization energy, very unreactive, low boiling and melting points Melting point, boiling point, density and atomic radius increase going down
46
Balmer spectral lines
Series of spectral lines of the hydrogen atom occur as the electrons transition from higher PEL to lower PEL at a principal quantum number of 2
47
Balmer equation
Wavelength = R (1/4 - 1/n^2) R= 1.097* 10^7 m^-1
48
Paschen spectral lines
Wavelength = R (1/9 - 1/n^2) Infared
49
Lyman series
Wavelength = Rh (1/n1^2 - 1/n2^2) Rh= 1.0974 * 10^-2 nm Ultraviolet
50
Paschan
Electrons falling into 3rd PEL
51
Balmer
Electrons falling into 2nd PEL
52
Lyman
Electrons falling into 1st PEL

AP Chem (5 decks)

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