Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

ADV. INORG CHEM > INORG. CHEM BASICS > Flashcards

INORG. CHEM BASICS Flashcards

1
Q

Father of Modern Periodic table

organized elements by their atomic weights and grouped them based on their chemical properties

A

Dmitri Ivanovich Mendeleev

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

number of a chemical element; is defined as the number of protons present in the nucleus; denoted by the symbol Z

A

Atomic number

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

defined as the total number of protons and neutrons in the nucleus of an atom; denoted by the symbol A

A

Mass number

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

the difference between the number of protons and numbers of electrons; denoted by the symbol n

A

Charge

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

aka chemical symbols/atomic symbols; one or two letter notations used to represent chemical elements; denoted by the symbol E

A

Element symbol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the structure of an atom?

A

Electron orbits
Nucleus
Proton
Neutron
Electrons

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

describes how electrons are distributed in its atomic orbitals

A

Electron configuration

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

indicates the main energy level of orbitals and electron

A

Principal Quantum number (n)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

indicates the energy sublevel, which is given by the type of the orbital

A

Angular Momentum Quantum Number (l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

indicates the specific orbital within the energy sublevel

A

Magnetic Quantum Number (ml)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

shows the direction of the electron spin

A

Electron Spin Quantum Number

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

electrons fill the orbitals in the order of increasing their energy level

A

Aufbau principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

no two electrons in an atom can have the same four quantum numbers

A

Pauli Exclusion Principle

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

electrons fill a subshell singly before forming any pairs and each electron in a single occupied orbital has the same spin

A

Hund’s rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Periodic table groups

A

1A = Alkali metals
2A = Alkali earth metals
3A = Boron group
4A = Carbon group
5A = Nitrogen group
6A = Chalcogens
7A = Halogens
8A = Noble gases
3d-6d = Transition metals
4f = Lanthanides
5f = Actinides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the periodic properties of atoms?

A
  1. Ionization energy
  2. Electron affinity
  3. Covalent and Ionic Radii
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Ionization potential; the energy requires to remove an electron from a gaseous atom or ion.

A

Ionization energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

An increase in ionization energy as the nuclear charge increases.

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

can be defined as the energy required to remove an electron from a negative ion

A

Electron affinity

ps: dearest ysa, please rest so research on this later

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

half the distance between two atoms that share a covalent bond

A

Covalent radius

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

these are the forces that exists between molecules

weaker than intramolecular forces

A

Intermolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

these are forces that exists within molecules

A

Intramolecular forces

23
Q

Common types of intermolecular forces:

A

Ion-dipole
Dipole-dipole
Hydrogen bonding
London dispersion

24
Q

chemically inert; does not form bonds with other atoms; released through the decay of Potassium; with weak London dispersion forces

A

Argon (.96%)

25
Q

exists as a diatomic molecule; inert gas; produced by the breakdown of ammonia; has a covalent bond

most abundant gas found in the earth’s atmosphere

A

Nitrogen (78%)

26
Q

produced from respiration and combustion; slightly strong intermolecular forces

A

Carbon dioxide (0.04%)

27
Q

diatomic molecule; produced by photosynthesis; more reactive than nitrogen; non-polar; less weak London dispersion force than nitrogen.

A

Oxygen (21%)

28
Q

Common types of intramolecular force:

A

Ionic bonds
Covalent bonds
Metallic bonds

29
Q

a type of chemical bond that involves the sharing of electron pairs between atoms

A

Covalent bonds

30
Q

unequal sharing if valence electrons resulting to partial positive charge on one atom and partial negative charge on the other

A

Polar covalent bond

31
Q

equal sharing of valence electron

A

Nonpolar covalent bond

32
Q

one atom transfers electrons to another atom; typically occurs between metals and non-metals

Properties:
High BP and MP; soluble in water

A

Ionic bond

33
Q

binds metal atoms together in a metallic substance; atoms are tightly packed together in a regular pattern; free moving electrons form clouds to promotes thermal and electrical conductivity

Properties:
High BP and MP
Good conductor of heat and electricity
Malleability and ductility

A

Metallic bond

34
Q

only one pair of electrons are shared between atoms; most stable but weak

A

Single bond

35
Q

two pair of electrons sharing between the involved the atoms; less stable but stronger

A

Double bond

36
Q

three pairs of electrons are shared between atoms; less stable but strongest

A

Triple bond

37
Q

a simplified representation of the valence of the valence shell electrons in a molecule

A

Lewis structures

38
Q

provides a method for predicting the shape of the molecules based on the electron-pair repulsion

lone pair electrons have the maximum repulsion, and the bonding pair electrons have the least repulsion

A

VSEPR

39
Q

predicts the structure based on the electron arrangements around the central atoms; steric number of a molecule

SN = bonding atoms attached to the central atom + lone pairs

A

Electron-domain geometry

40
Q

is the experimental distinction of the shape of a molecule or a polyatomic ion

A

Molecular geometry

41
Q

the mixing of atomic orbitals in atom (usually a central atom) to generate a set of hybrid orbitals

A

Hybridization

42
Q

atomic orbitals obtained when two or more nonequivalent (search meaning lol) orbitals of the same atom combine in prep. for covalent bond formation

A

Hybrid orbitals

43
Q

is the symmetrical three-dimensional structural
arrangements of atoms, ions or molecules (constituent particle)
inside a crystalline solid as points

A

Crystal lattice

44
Q

the simplest repeating unit which is consists of lattice points that
represent the locations of atoms or ions

A

Unit cell

45
Q

Each corner of
the cube has one atom, resulting in
a relatively low packing efficiency.

A

Simple cubic (SC)

46
Q

Has one atom at each corner and one
atom in the center of the cube. This
structure has higher packing efficiency than the simple cubic.

A

Body-centered cubic (BCC)

47
Q

A structure where layers of atoms are
stacked in an ABAB pattern, resulting
in a very efficient packing.

A

Hexagonal close-packed (HCP)

48
Q

Has one atom at each corner and one
atom in the center of each face of
the cube, leading to a very dense packing

A

Face-centered cubic (FCC)

49
Q

These are other crystal systems where
the unit cell dimensions and angles
vary, leading to different packing
efficiencies and symmetries

A

Tetragonal, Orthorhombic,
Monoclinic, Triclinic, Rhombohedral

50
Q

provides
recommendations on the nature and use of chemical nomenclature.

A

The International Union of Pure and Applied Chemistry (IUPAC)

51
Q

provides
information only on the composition of an ion, molecule, or compound.

A

Stoichiometric or compositional name

52
Q

where only one element is present, the name is formed by combining the
element name with the appropriate multiplicative
prefix

A

homoatomic entities

53
Q

(those containing atoms
of two elements) are named stoichiometrically
by combining the element names and
treating, by convention, the element reached
first when following the arrow in the element
sequence (Figure 1) as if it were an anion.

A

Binary compounds

54
Q

in general can be
named similarly using compositional
nomenclature, but often either substitutive or
additive nomenclature is used

A

Heteropolyatomic entities

ADV. INORG CHEM (4 decks)

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