INORG. CHEM BASICS Flashcards
Father of Modern Periodic table
organized elements by their atomic weights and grouped them based on their chemical properties
Dmitri Ivanovich Mendeleev
number of a chemical element; is defined as the number of protons present in the nucleus; denoted by the symbol Z
Atomic number
defined as the total number of protons and neutrons in the nucleus of an atom; denoted by the symbol A
Mass number
the difference between the number of protons and numbers of electrons; denoted by the symbol n
Charge
aka chemical symbols/atomic symbols; one or two letter notations used to represent chemical elements; denoted by the symbol E
Element symbol
What is the structure of an atom?
Electron orbits
Nucleus
Proton
Neutron
Electrons
describes how electrons are distributed in its atomic orbitals
Electron configuration
indicates the main energy level of orbitals and electron
Principal Quantum number (n)
indicates the energy sublevel, which is given by the type of the orbital
Angular Momentum Quantum Number (l)
indicates the specific orbital within the energy sublevel
Magnetic Quantum Number (ml)
shows the direction of the electron spin
Electron Spin Quantum Number
electrons fill the orbitals in the order of increasing their energy level
Aufbau principle
no two electrons in an atom can have the same four quantum numbers
Pauli Exclusion Principle
electrons fill a subshell singly before forming any pairs and each electron in a single occupied orbital has the same spin
Hund’s rule
Periodic table groups
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
What are the periodic properties of atoms?
- Ionization energy
- Electron affinity
- Covalent and Ionic Radii
Ionization potential; the energy requires to remove an electron from a gaseous atom or ion.
Ionization energy
An increase in ionization energy as the nuclear charge increases.
can be defined as the energy required to remove an electron from a negative ion
Electron affinity
ps: dearest ysa, please rest so research on this later
half the distance between two atoms that share a covalent bond
Covalent radius
these are the forces that exists between molecules
weaker than intramolecular forces
Intermolecular forces
these are forces that exists within molecules
Intramolecular forces
Common types of intermolecular forces:
Ion-dipole
Dipole-dipole
Hydrogen bonding
London dispersion
chemically inert; does not form bonds with other atoms; released through the decay of Potassium; with weak London dispersion forces
Argon (.96%)
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
Nitrogen (78%)
produced from respiration and combustion; slightly strong intermolecular forces
Carbon dioxide (0.04%)
diatomic molecule; produced by photosynthesis; more reactive than nitrogen; non-polar; less weak London dispersion force than nitrogen.
Oxygen (21%)
Common types of intramolecular force:
Ionic bonds
Covalent bonds
Metallic bonds
a type of chemical bond that involves the sharing of electron pairs between atoms
Covalent bonds
unequal sharing if valence electrons resulting to partial positive charge on one atom and partial negative charge on the other
Polar covalent bond
equal sharing of valence electron
Nonpolar covalent bond
one atom transfers electrons to another atom; typically occurs between metals and non-metals
Properties:
High BP and MP; soluble in water
Ionic bond
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
Metallic bond
only one pair of electrons are shared between atoms; most stable but weak
Single bond
two pair of electrons sharing between the involved the atoms; less stable but stronger
Double bond
three pairs of electrons are shared between atoms; less stable but strongest
Triple bond
a simplified representation of the valence of the valence shell electrons in a molecule
Lewis structures
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
VSEPR
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
Electron-domain geometry
is the experimental distinction of the shape of a molecule or a polyatomic ion
Molecular geometry
the mixing of atomic orbitals in atom (usually a central atom) to generate a set of hybrid orbitals
Hybridization
atomic orbitals obtained when two or more nonequivalent (search meaning lol) orbitals of the same atom combine in prep. for covalent bond formation
Hybrid orbitals
is the symmetrical three-dimensional structural
arrangements of atoms, ions or molecules (constituent particle)
inside a crystalline solid as points
Crystal lattice
the simplest repeating unit which is consists of lattice points that
represent the locations of atoms or ions
Unit cell
Each corner of
the cube has one atom, resulting in
a relatively low packing efficiency.
Simple cubic (SC)
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.
Body-centered cubic (BCC)
A structure where layers of atoms are
stacked in an ABAB pattern, resulting
in a very efficient packing.
Hexagonal close-packed (HCP)
Has one atom at each corner and one
atom in the center of each face of
the cube, leading to a very dense packing
Face-centered cubic (FCC)
These are other crystal systems where
the unit cell dimensions and angles
vary, leading to different packing
efficiencies and symmetries
Tetragonal, Orthorhombic,
Monoclinic, Triclinic, Rhombohedral
provides
recommendations on the nature and use of chemical nomenclature.
The International Union of Pure and Applied Chemistry (IUPAC)
provides
information only on the composition of an ion, molecule, or compound.
Stoichiometric or compositional name
where only one element is present, the name is formed by combining the
element name with the appropriate multiplicative
prefix
homoatomic entities
(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.
Binary compounds
in general can be
named similarly using compositional
nomenclature, but often either substitutive or
additive nomenclature is used
Heteropolyatomic entities
