Bonding and IMF, and Atomic Nucelus Flashcards
ionic and covalent bonds are
intramolecular forces
any force that binds together the atoms making up a molecule or compound
Name the intramolecular force
strong chemical bonds that hold together ions of the opposite charge
ionic bonds
In ionic bonds, electrons are completely transferred from one species to another, forming the cation and anion. This transfer occurs between species that have significant differences in electronegativities
rank the intramolecular forces from strongest to weakest
- ionic
- polar covalent
- non-polar covalent
Name the intramolecular force
the sharing of an electron pair between two atoms
covalent bond
can be polar or non-polar
e.g Cl2, O2
Name the intramolecular force
form between atoms that have similar or identical electronegativity values when the electrons are shared equally
non-polar covalent bonds
equal to or less than 0.5 electronegativity
Name the intramolecular force
bonds that form between atoms with a moderate electronegativity difference that share electrons
polar covalent
0.5 to 1.7 electronegativity difference
Note: the sharing of these electrons is unequal; there is a moderate dipole
E.g HCl, H2O
Define
the number of bonding pairs of electrons between two atoms
bond order
In a covalent bond between two atoms, a single bond has a bond order of one, a double bond has a bond order of two, a triple bond has a bond order of three, and so on
Name the term
a bond formed when atomic orbitals are parallel to each other but perpendicular to the internuclear axis, forming a weaker side-to-side interaction
pi (𝝅) bond
Think: parallel
a bond formed by the overlap of two orbitals in an end-to-end fashion along the internuclear axis
sigma bond
A single bond contains how many pi and sigma bonds?
1 sigma bond
A double bond contains how many pi and sigma bonds?
1 sigma and 1 pi
A triple bond contains how many pi and sigma bonds?
1 sigma and 2 pi
How is bond length related to bond order
They are inversely related
the energy required to break a covalent bond between two atoms
bond energy
the higher the bond energy, the stronger the bond
Bond energy increases as bond order increases
chemical bonding between tmetal atoms, which arises from the attraction between positively charged metal nuclei and their delocalized valence electron
metallic bonding
electrons are delocalized and are attracted to multiple nuclei, creating a “sea of electrons” that are free to move throughout the solid
What type of bonding accounts for the phyiscal properties of metals?
metallic bonding
The freedom of electron movement accounts for the ability of metals to conduct heat and electricity, gives metals their luster, and makes them malleable
Rank the intermolecular forces from strongest to weakest
- ion-dipole
- hydrogen bonding
- dipole-dipole
- london dispersion
True or False
Intermolecular forces are stronger than intramolecular forces
False
bonds between molecules are notably weaker than those within a molecule
____ means within a molecule, and ____ means between molecules
intra, inter
dipole-dipole interactions
London dispersion
Hydrogen bonding
Ion dipole interactions
State the equation to calculate formal charge
FC = VE - 1/2 BE - LPE
valence electrons - (covalent bonds - lone pair electrons)
What do these equations represent?
alpha decay
nuclear decay process where an unstable nucleus changes to another element by shooting out a particle composed of two protons and two neutrons
alpha decay
a radioactive decay in which a ____ ray is emitted from an atomic nucleus, raising the atomic number of the atom by one if the particle is negatively charged, lowering it by one if positively charged.
beta decay
beta decay
Name the two types of beta decay:
One type (____) releases a positively charged beta particle called a positron, and a neutrino; the other type (____) releases a negatively charged beta particle called an electron, and an antineutrino
beta plus, beta minus
Name the type of decay
the nucleus emits radiation without actually changing its composition; there is no change in an atomic number
gamma decay
