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AP Chemistry > Unit 1 - Atomic Structure & Properties > Flashcards

Unit 1 - Atomic Structure & Properties Flashcards

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1
Q

What is formula mass?

A

The mass of one of basic unit in a network solid

Expressed in amu

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2
Q

What is molecular mass

A

The mass of molecules that can exist independently

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3
Q

How do you determine the molar mass for a molecule?

A

Add up the corresponding masses on the periodic table.

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4
Q

What is the Avogadro’s number?

A

Number that indicates the number of molecules or atoms in one mole of a substance (6.022 * 10 ^23 mole^-1)

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5
Q

What is a mole?

A

The fundamental unit for counting particles on the macroscopic level

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6
Q

How do you determine the number of moles with a given mass?

A

Multiply that amount of mass by the reciprocal of the molar mass.

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7
Q

What is the nucleus made up of?

A

Neutrons (no charge) and protons (positive charge)

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8
Q

What are the electron shell?

A

The layers of electrons orbiting the nucleus composed of largely empty space

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9
Q

What is the mass number?

A

Equals to the number of protons and neutrons of an element (e.g. C has a mass number of 12)

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10
Q

What is the atomic number?

A

Equals to the number of protons in a neutral atom (e.g. C has an atomic number of 6)

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11
Q

What is an isotope?

A

Forms of an element that has the same number of protons with differing number of neutrons which exhibits identical chemical properties

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12
Q

What is average atomic mass?

A

Average of the masses of all the isotopes of an element based on their proportion

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13
Q

What is mass spectroscopy used for?

A

To compare the masses of isotopes through a process of ionization and acceleration through a magnetic field; lighter isotopes will have a greater degree of deflection

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14
Q

What is a pure sample?

A

A sample with only particles of one type of atom, molecule, or formula unit

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15
Q

What is a mixture?

A

A substance that contains particles of more than one type of atoms, formula unit, or molecules not chemically combined

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16
Q

What is the Law of Definite Proportion?

A

Different pure samples of the same compound will always contain the same proportions of each element by mass

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17
Q

What is mass percent?

A

Percent by mass of an element in a pure sample of a compound in a substance

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18
Q

How to calculate mass percent?

A

Mass percent of A = (# of atoms) (A’s atomic mass) / formula weight of a compound * 100
Mass percent of component = (mass of component) / total mass of substance * 100

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19
Q

What is molecular formula?

A

Chemical formula that provide actual number of each type of atom in a molecule

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20
Q

What is empirical formula?

A

Chemical formula that provides the relative number of each type of atom in molecule (ratio in the simplest form)

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21
Q

How do you determine the multiplier for the empirical formula?

A

molar mass divided by the empirical formulas molar mass

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22
Q

What is the usage of combustion analysis?

A

To analyze the composition of hydrocarbons; carbon composition can be determined by mass of CO2 produced, hydrogen can be determined by the mass of H2O produced, and oxygen can be determined by the difference after C and H have been determined

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23
Q

What are orbits?

A

Space where electrons move around; only certain orbits exist w/fixed distance away from nucleus

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24
Q

What is the Couloub’s Law?

A

F= k * q1q2/d^2 q= magnitude of charge associated with a particle d= distance between charged particles

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25
Q

What is the shielding effects?

A

Electrons located further away from the nucleus are partially shielded by inner core electrons due to electrostatic repulsion.

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26
Q

What is the first ionization energy?

A

Minimum amount of energy required to remove an outermost, least tightly held electrons from an atom in the gas phase

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27
Q

What is an orbital?

A

Wave function that describes an electron’s possible positions in 3-D space

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28
Q

What are the 4 possible orbital types and electrons held in each

A

S- 2
P- 6
D- 10
F- 14

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29
Q

What are isoelectronic species?

A

Species that share the same electronic configuration but have different radii

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30
Q

What are d-block cations?

A

Elements in the d-block that lose elements from highest s-sublevels before losing from d-sublevel

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31
Q

What is the Aufbau Principle?

A

Each orbital can hold max of two electrons spinning in opposite directions

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32
Q

What is the Hund’s Rule?

A

When you have more than one orbital in a subshell, a single spin up electron is added to each orbital before you start adding spin down electrons.

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33
Q

What is the relationship between first ionization energy and shielding effect?

A

As average distance increases between the nucleus and electrons, the lower the first ionization energy due to the shielding effect.

34
Q

What does PES data correspond with?

A

PES data corresponds with the theory that each electron shell contain subshells.

35
Q

What is the effective nuclear charge?

A

Nuclear charge experienced by an electron

36
Q

Inner core electrons

A

contained in the inner shells

37
Q

Valence electrons

A

contained in the outer shells

38
Q

First ionization energy pattern in periodic table

A

Increases as we move from left to right

Decreases as we move from top to bottom

39
Q

Ionization data suggests that

A

electrons are arranged in shells

40
Q

Electron configuration

A

Notation to write the number of electrons found in chemical species in accordance with orbitals

41
Q

As the ratio of protons to electrons increases, the forces of attraction on those electrons

A

increase

42
Q

Example of d-block cations

A

Fe2+ [Ar] 3d^6

43
Q

n = 1 contains

A

one subshell – 1s

max of 2 electrons

44
Q

n = 2 contains

A

two subshells – 2s and 2p

max of 8 electrons

45
Q

n = 3 contains

A

three subshells – 3s, 3p, and 3d

max of 18 electrons

46
Q

n = 4 contains

A

four subshells – 4s, 4p, 4d, and 4f

max of 32 electrons

47
Q

2p electrons experience a
greater shielding effect
from the 1s electrons than

A

do the 2s electrons.

48
Q

the more effectively the electrons within a sub-shell are able to penetrate the
shielding electrons, the greater the

A

ionization energy of those electrons.

49
Q

Periodicity

A

Predictable physical and chemical trends that
occur as one moves across a period or down a
group in the periodic table.

50
Q

Atomic Radius

A

Increases down a group
New shells added, valence electrons are less stable, shielding, greater distance

Decreases across a period
Addition of protons, valence electrons in same shell

51
Q

Metals lose electrons to form

A

cations

52
Q

Nonmetals gain electrons to form

A

anions

53
Q

Ionic radius

A

Cations are smaller than neutral atoms

Anions are larger than neutral atoms

54
Q

Ionic Radius of Cations

Across a Period from Left to Right

A

Radii of cations decrease

protons added -> increases force of attraction, increase effective nuclear charge

55
Q

Ionic Radius of Anions

Across a Period from Left to Right

A

When you encounter the first anion, the radius
increases dramatically -> expansion of electron cloud

The radii then continue to decrease
protons added -> increases force of attraction, increase effective nuclear charge

56
Q

First Ionization Energy exceptions

A

It requires more energy to pull an electron from a full
d-subshell than it does to pull the only electron in a
p-subshell (when in the same period).
• It requires more energy to pull an electron from a full s-subshell than it does to pull the only electron in a p-subshell (when in the same period).
– That single electron is easier to remove

57
Q

The second ionization potential for an atom is

always

A

greater than the first.

58
Q

Every element has one extremely large increase in

ionization energy. This occurs when

A

electron configuration drops a

principal quantum number

59
Q

Electron Affinity

A

The energy change that occurs when an electron is
added to a gaseous atom to form a negative ion.

a measure of how much an element wants to
accept another electron.

60
Q

If electron affinity is negative, then it

A

Releases energy -> exothermic

Wants to accept electron

61
Q

If electron affinity is positive, then it

A

Requires energy -> endothermic

Does not want to accept electron

62
Q

Electron Affinity pattern

A

Increases as we move from left to right
protons added -> increases force of attraction, increase effective nuclear charge

Increases as we move from bottom to top
Larger distance between nucleus and valence electron = less energy

63
Q

Electron affinity is always positive for elements in

A

Group 2A and 8A
Highest energy subshell is full
Added electron would be only electron in higher shell -> requires a lot of energy to overcome repulsion

64
Q

Electronegativity

A

An element’s ability to attract electrons in a

chemical bond

65
Q

Electronegativity pattern

A

Increases from left to right

Increase from bottom to top

Increases as atomic radius decreases

66
Q

Octet Rule

A

Elements tend to gain, lose, or share valence electrons to acquire a full octet

Exception - element in period 1 has a full octet of 2 electrons

67
Q

Metals and non-metals loses electrons to obtain

A

a full octet

68
Q

Ionic compounds are formed when

A

metal cations form electrostatic bonds with non-metal anions.

69
Q

Ionic Bonding

A

1-Metals transfer electrons to non-metals and form bonds due to electrostatic attractions

2-Cations and anions form electrostatic bonds based on opposite charges

70
Q

Recognizing Ionic Compounds

A

Contain either a metal and a non-metal or polyatomic ions

First word in compound name is metal/ammonium

71
Q

Naming Ionic Compounds

A

The positive ion (cation) is written first and takes the same name as the element.

The negative ion (anion) is written last and takes the first part of its elements name and –ide is added to the end.

72
Q

Some metals can forms cations with

A

different charges

73
Q

Roman numerals indicate the

A

Charge that is carried by the cation when that metal is able to form cations with different charges

74
Q

Copper(I) sulfide contains

A

Cu+ cations

75
Q

Copper(II) sulfide contains

A

Cu2+ cations

76
Q

Cations with alternate forms include

A

Copper -> Cu+ or Cu2+
Iron -> Fe2+ or Fe3+
Lead -> Pb2+ or Pb4+

77
Q

Most polyatomic ions do not have an

A

-ide suffix

78
Q

Only three polyatomic ions end in -ide

A

CN- Cyanide
OH- Hydroxide
O2 2- Peroxide

79
Q

Only polyatomic cation need to know about is

A

Ammonium NH4+

80
Q

When writing ionic formulas, keep in mind

A

Ionic compounds are neutral -> all charges sum up to zero

Charges come from associated group in periodic table or list

Parentheses must be used when there is some multiple of a certain polyatomic ion

81
Q

Charges on ions relate to

A

group they’re in

82
Q 
Group 1A 
Group 2A  
d-block
Group 3A 
Group 4A  
Group 5A  
Group 6A 
Group 7A
A 
\+1 (H can also be –1)
\+2
\+1 to +5 (it s’ hard to predict)
\+3 (Tl can also be +1)
\+4 (Sn and Pb can also be +2)
-3 non-metals, +3 and +5 metals
-2 non-metals, +2 and +4 metals
 -1

AP Chemistry (9 decks)

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