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AP Chem > Chapter 7 > Flashcards

Chapter 7 Flashcards

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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
Q

Electron affinity

A

The change in energy of kJ per mole in a neutral atom while an electron is added to make a negative ion

25
Q

Why does oxygen require energy to add 2nd electron?

A

Electrons out number protons, the nucleus does not attract electrons as strongly and the electrons repel eachother

26
Q

Electron affinity trends

A

Increases across a period

Decreases down a group

27
Q

Exceptions to electron affinity rules

A

Noble gases, group 5 metals and group 2 metals require energy to add an electron because they’re already stable

28
Q

Metallic character

A

How closely relatable the element is to the standard properties of a metal

29
Q

Metallic character trends

A

Decreases across a period

Increases down a group

30
Q

Nonmetallic character

A

How closely relatable the element is to the standard properties of a nonmetal

31
Q

Metal characteristics

A 
Luster,
Solid 
Malleable and ductile
Good conductors
Form positive ions 
Ionic bonding
32
Q

Nonmetal characteristics

A 
No luster
Generally gases
Brittle
Poor conductors
Covalent bonds
Negative ions
33
Q

Metalloids

A

Elements that have both metal and nonmetal properties

34
Q

Alkali metal characteristics

A 
Silver luster 
Behaves as metals
High conductivities
Low melting and boiling points
Reactive (active metals
Exothermic
Colorless until set on fire
35
Q

Water as a reactive ion (alkali metals)

A

Forms hydrogen gas and alkali metal hydroxides
Exothermic reactions
Violent reactions with heavy metals

36
Q

Oxygen ion as a reactive ion (alkali metals)

A

Complex reactions
Lithium forms oxides
Sodium forms peroxides
Potassium, rubidium and cesium form superoxides

37
Q

Alkali metal trends (down group)

A

Melting point decreases
Densities increase
Become softer
Reactivity increases

38
Q

Alkaline earth metal characteristics

A 
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
Q

Alkaline earth metal trends going down a group

A

Ease of losing electrons increases

Reactivity increases

40
Q

Water as a reactive ion (alkaline earth)

A

Mg reacts with steam
Na and K react with water
Ca reacts with hot water
Forms hydrogen gas and hydroxide

41
Q

Nonmetals as reactive ions (alkaline earth)

A

Loses two electrons in a sublevel
Magnesium is least reactive
Heavier= more reactive

42
Q

Hydrogen characteristics

A

Colorless, odorless, lowest density

More than double ionization energy compared to other metals, properties of metal and nonmetal

43
Q

Oxygen group (chalcogens) trends

A

Melting point, boiling point, ionization energy, electro negativity, density, atomic radius, toxicity and ionic radius increase as you go down

44
Q

Halogens characteristics

A

Poor conductors, low melting and boiling points, forms ionic salts, highly reactive, decrease down a group, easily dissociate

45
Q

Noble gases characteristics

A

Colorless, monoatomic, large ionization energy, very unreactive, low boiling and melting points

Melting point, boiling point, density and atomic radius increase going down

46
Q

Balmer spectral lines

A

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
Q

Balmer equation

A

Wavelength = R (1/4 - 1/n^2)

R= 1.097* 10^7 m^-1

48
Q

Paschen spectral lines

A

Wavelength = R (1/9 - 1/n^2)

Infared

49
Q

Lyman series

A

Wavelength = Rh (1/n1^2 - 1/n2^2)

Rh= 1.0974 * 10^-2 nm

Ultraviolet

50
Q

Paschan

A

Electrons falling into 3rd PEL

51
Q

Balmer

A

Electrons falling into 2nd PEL

52
Q

Lyman

A

Electrons falling into 1st PEL

AP Chem (5 decks)

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