Atomic and Molecular Structure Flashcards
Dalton’s atomic theory explains that all matter is made up of -__ which are ___. And that all atoms of a given element are identical in __ and ___
atoms, indivisible, mass, property
___ electrons are all electrons except the valence electrons, and the number of electrons in each energy level is equal to ____
core, 2n^2
atoms of the same element that have the same number of protons but different number of neutrons
isotopes
involves changes to the physical properties of a substance; no new products are formed and no new chemical bonds are formed or destroyed
physical reactions
When bonds are formed or broken and new substances are made
chemical reaction
When two different compounds come together to form a single compound; usually release energy
synthesis
When a compound breaks down into two or more products; require energy
decomposition
When one element replaces another in a compound
single displacement
When two elements replace one another in a compound
double displacement
When a substance reacts with O2 to form light and heat
combustion
Bohr believed that electrons move in __ __ around the nucleus, but this has since been disproven
fixed orbitals
states that it is impossible to know both the exact location and momentum of an electron at the same time
heisenberg’s uncertainty principle
the space that is the most probable locations for electrons
electron cloud
The __ ___ ___ describes the energy level of the electron, and it must be ____. The maximum number of electrons each level can hold is given by ____. The ___ number on the periodic table represents the energy level of the valence electrons
principle quantum number, N>=1, 2n^2, row
the __ __ __ describes the orbital shape, and can be between __ and ___.
azimuthal quantum number, 0, n-1
When l = 0, the subshell is ___, which is ___ shaped, when l=1 the subshell is ___ which is ____ shaped, when l=2 the subshell is ____ which is ___ shaped and when l=3, the subshell is ___
s, spherical p, dumbell, d, clover, f
The magnetic quantum number describes the __ ___ in space, and takes the value of __ and ___
orbital orientation, -l, +l
The __ ___ __ describes the angular momentum of the electron and can be either __ or ___
spin quantum number, -1/2, +1/2
Says that no two electrons within an atom can have the exact same quantum numbers
pauli’s exclusion principle
The s orbital has __ electrons, the p orbital has ___ electrons, the d orbital has ___ electrons, and the f orbital has ___ electrons
2, 6, 10, 14
describes the number of electrons in each energy level and the order in which subshells are filled
electron configuration
In electron configuration notation, the first number describes the __ __ __, and the letter describes its ___, the superscript describes the number of ___ in it
principle energy level, subshell, electrons
the alkali and alkaline earth metals are the ___ block, the nonmetals are the ___, the transition metals are the __, and the lanthinide and actinides are the ___ block
s, p, d, f
says that subshells tend to get filled from lower energy to higher energy
aufbau principle
Says that all orbitals of a subshell are first singly occupied before they are doubly occupied
hund’s rule
Exceptions to the electron configurations occur when elements like to have ___ or ___ ___ subshells. This includes elements like __, __ and ___, ___, ___
full, half full, Cr, Mo, Au, Ag, Cu
Valence electrons are always removed first from the __ ____ subshell
highest energy
When two species that have the same electronic configurations
isoelectronic species
Ionic compounds are ___ __ that have high melting and __ ___, are soluble in ___, and __ __ in aqueous and __ forms
crystalline solids, boiling points, water, conduct electricity, molten
Covalent compounds have weaker bonds than ionic, thus have lower _- and ___ points, are ___ or ___ at room temperature, are __ in water, and do not conduct ___
melting, boiling, liquid, gas, insoluble, electricity
distance between the each atom in a covalent bond; decreases as the number of electron pairs shared increases
bond length
The energy needed to break the covalent bond; increases as the electron pairs shared increases
bond energy
distribution of charges
polarity
When atoms of a chemical compound are covalently bonded in a network
covalent network solid
Examples of covalent network solids are __ and ___
diamond, quartz
When in a covalent bond, both electrons come from the same atom
coordinate covalent
electrostatic attractive force between delocalized electrons and positively charged metal ions
metallic bond
Metallic compounds like __ and __ fused together, conduct ___, are ___, ___, and ___
gold, silver, electricity, ductile, malleable, lustrous
dipole dipole interactions does not occur in ____ because the molecules are too far apart.
gasses
Ion dipole interactions are the attraction between the ____ and ___ molecules, and are stronger than dipole dipole interactions,
ions, polar
Increasing the intermolecular forces increases the __ and __ points, the ___, the __ __, and decreases the __ ___
melting, boiling, viscosity, surface tension, vapor pressure
The __ ___ rule applies to hydrogen, helium, ____, ____, ___ and -__
reduced octet, lithium beryllium, boron, aluminum
___ ___ is when elements have more than 8 outer electrons and apply to elements within the __ row or more that have a __ subshell
exceeding octet, 3rd, d
the central atom is the one that can make the most __, and is usually the __ ___ atom. It is also usually ___
bonds, least electronegative, carbon
___ and ___ will never be the central atom, and will only form one bond.
hydrogen, halogens
the formula for formal charge
number of valence electrons - non bonding electrons - number of bonds
Bonding occurs when orbitals with electrons ___. When this happens, the atomic orbitals are ____ into shapes that resemble the atomic orbitals. This forms a __ ___. The number of orbitals must be ___. Hybrid orbitals have better __ and form ___ bonds
overlap, hybridized, covalent bond, conserved, overlap, stronger
sigma bonds allow for __ __ about its axis, whereas ___ bonds do no
free rotation, pi
All single bonds are ___ bonds. A double bond has ___ pi bond and a triple bond has ___ pi bonds
sigma, 1, 2
the number of lone pairs or bond locations around an atom
number of lone pairs or bond locations around an atom
Double and triple bonds only count as ___ electron domain
1
The bond order is equal to
number of bonding orbital electron - number of antibonding orbital electron / 2
bond order is equal to the number of ___
bonds
an atom that has one or more unpaired electrons and thus is attracted to a magnetic field
paramagnetic
when an element has no unpaired electrons and thus repels a magnetic field
diamagnetic
As the bond order increases, the bond strength ____. An increase in ___ __ produces a decrease in bond strength. The greater the ____, the greater the bond strength. The presence of less ___ ___ indicates a greater bond strength
increase, atomic radii, polarity, lone pairs
VSPER theory determines the __ __ of ___ molecules. Electron pairs ___ each other and will arrange themselves as far apart as possible
geometric arrangement, covalent, repel,
has 2 electron domains and 180° separation
linear
has 3 electron domains and 120° separation
trigonal planar
has 4 electron domains and 109.5° separation
tetrahedral
Has 5 electron domains with 90°, 180°, and 120° separations
trigonal bipyramidal
Has 6 electron domains with 90° separation
octahedral
a bent shape that occurs with ___ bonds and __ lone pair has a bond angle of ___ 120°
2, 1, <
a trigonal pyramidal shape that occurs due to ___ bonds and __ lone pair has a bond angle of ___
3, 1, 107.5°
The bent shape created by __ bonds and ___ lone pairs has a bond angle of ___
2, 2, 104.5°
a ____ shape is formed with 4 bonds and 1 lone pair, with angles that are greater than __ and ___
seesaw, 90, 120
A ____ shape results from 3 bonds and 2 lone pairs, and has a bond angle of ___90
t, <
a ___shape can result from a molecule of 2 bonds and 3 lone pairs, and has a bond angle of ___
linear, 180°
a ___ __ shape results from a molecule with 5 bonds and 1 lone pair and its bond angle is ____ 90
square pyramidal, <
A __ __ shape results from a molecule with 4 bonds and 2 lone pairs and has a bond angle of ____
square planar, 90°
