Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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

Unit 1 - Atomic Structure & Properties Flashcards

1
Q

What is formula mass?

A

The mass of one of basic unit in a network solid

Expressed in amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is molecular mass

A

The mass of molecules that can exist independently

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How do you determine the molar mass for a molecule?

A

Add up the corresponding masses on the periodic table.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is a mole?

A

The fundamental unit for counting particles on the macroscopic level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the nucleus made up of?

A

Neutrons (no charge) and protons (positive charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are the electron shell?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is average atomic mass?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is a pure sample?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is mass percent?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is molecular formula?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How do you determine the multiplier for the empirical formula?

A

molar mass divided by the empirical formulas molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What are orbits?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is the shielding effects?
Electrons located further away from the nucleus are partially shielded by inner core electrons due to electrostatic repulsion.
26
What is the first ionization energy?
Minimum amount of energy required to remove an outermost, least tightly held electrons from an atom in the gas phase
27
What is an orbital?
Wave function that describes an electron's possible positions in 3-D space
28
What are the 4 possible orbital types and electrons held in each
S- 2 P- 6 D- 10 F- 14
29
What are isoelectronic species?
Species that share the same electronic configuration but have different radii
30
What are d-block cations?
Elements in the d-block that lose elements from highest s-sublevels before losing from d-sublevel
31
What is the Aufbau Principle?
Each orbital can hold max of two electrons spinning in opposite directions
32
What is the Hund's Rule?
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.
33
What is the relationship between first ionization energy and shielding effect?
As average distance increases between the nucleus and electrons, the lower the first ionization energy due to the shielding effect.
34
What does PES data correspond with?
PES data corresponds with the theory that each electron shell contain subshells.
35
What is the effective nuclear charge?
Nuclear charge experienced by an electron
36
Inner core electrons
contained in the inner shells
37
Valence electrons
contained in the outer shells
38
First ionization energy pattern in periodic table
Increases as we move from left to right | Decreases as we move from top to bottom
39
Ionization data suggests that
electrons are arranged in shells
40
Electron configuration
Notation to write the number of electrons found in chemical species in accordance with orbitals
41
As the ratio of protons to electrons increases, the forces of attraction on those electrons
increase
42
Example of d-block cations
Fe2+ [Ar] 3d^6
43
n = 1 contains
one subshell – 1s | max of 2 electrons
44
n = 2 contains
two subshells – 2s and 2p | max of 8 electrons
45
n = 3 contains
three subshells – 3s, 3p, and 3d | max of 18 electrons
46
n = 4 contains
four subshells – 4s, 4p, 4d, and 4f | max of 32 electrons
47
2p electrons experience a greater shielding effect from the 1s electrons than
do the 2s electrons.
48
the more effectively the electrons within a sub-shell are able to penetrate the shielding electrons, the greater the
ionization energy of those electrons.
49
Periodicity
Predictable physical and chemical trends that occur as one moves across a period or down a group in the periodic table.
50
Atomic Radius
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
Metals lose electrons to form
cations
52
Nonmetals gain electrons to form
anions
53
Ionic radius
Cations are smaller than neutral atoms Anions are larger than neutral atoms
54
Ionic Radius of Cations | Across a Period from Left to Right
Radii of cations decrease | protons added -> increases force of attraction, increase effective nuclear charge
55
Ionic Radius of Anions | Across a Period from Left to Right
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
First Ionization Energy exceptions
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
The second ionization potential for an atom is | always
greater than the first.
58
Every element has one extremely large increase in | ionization energy. This occurs when
electron configuration drops a | principal quantum number
59
Electron Affinity
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
If electron affinity is negative, then it
Releases energy -> exothermic Wants to accept electron
61
If electron affinity is positive, then it
Requires energy -> endothermic Does not want to accept electron
62
Electron Affinity pattern
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
Electron affinity is always positive for elements in
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
Electronegativity
An element's ability to attract electrons in a | chemical bond
65
Electronegativity pattern
Increases from left to right Increase from bottom to top Increases as atomic radius decreases
66
Octet Rule
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
Metals and non-metals loses electrons to obtain
a full octet
68
Ionic compounds are formed when
metal cations form electrostatic bonds with non-metal anions.
69
Ionic Bonding
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
Recognizing Ionic Compounds
Contain either a metal and a non-metal or polyatomic ions First word in compound name is metal/ammonium
71
Naming Ionic Compounds
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
Some metals can forms cations with
different charges
73
Roman numerals indicate the
Charge that is carried by the cation when that metal is able to form cations with different charges
74
Copper(I) sulfide contains
Cu+ cations
75
Copper(II) sulfide contains
Cu2+ cations
76
Cations with alternate forms include
Copper -> Cu+ or Cu2+ Iron -> Fe2+ or Fe3+ Lead -> Pb2+ or Pb4+
77
Most polyatomic ions do not have an
-ide suffix
78
Only three polyatomic ions end in -ide
CN- Cyanide OH- Hydroxide O2 2- Peroxide
79
Only polyatomic cation need to know about is
Ammonium NH4+
80
When writing ionic formulas, keep in mind
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
Charges on ions relate to
group they're in
82
``` Group 1A Group 2A d-block Group 3A Group 4A Group 5A Group 6A Group 7A ```
``` +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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions