A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
What is a chemical bond?
The outermost electrons
What are the valence electrons?
Stored up energy
What is potential energy?
1. cation and anion electrical attraction
2. breaks apart easily
3. only happens between a metal and nonmetal
2. breaks apart easily
3. only happens between a metal and nonmetal
What is an ionic bonding?
1. sharing electrons
2. nonmetal and nonmetal
3. electrons are “owned” by both atoms
4. non-polar covalent: electrons shared equally, same elements
5. polar covalent: electrons shared unequally
2. nonmetal and nonmetal
3. electrons are “owned” by both atoms
4. non-polar covalent: electrons shared equally, same elements
5. polar covalent: electrons shared unequally
what is a covalent bond?
Neutral group of atoms that are covalently bonded
What is a molecule?
Types of elements and the number of elements
What are molecular formulas?
Distance between nuclei of two atoms that are bonded
What is bond length?
Energy required to break a bond
What is bond energy?
1. Strong bond
2. More energy to break it
2. More energy to break it
What does high bond energy mean?
made of positive and negative ions held by ionic bonding
Most rocks and minerals are
weaker
An ionic bond is much _________________ than covalent bonds
neutral charge
An ionic compound wants a ____________
A three-dimensional network of positive and negative ions
What is a crystal?
Looks at smallest whole number ratio of cations and anions
What is a formula unit?
Energy required to break a lattice (to dissolve)
What is lattice energy?
Forces of attraction between molecules of a covalent compound are much weaker
What are intermolecular forces?
Strength of intermolecular forces
What is melting point?
stronger intermolecular forces
Ionic compounds have much ____________________ than covalent compounds
1. High melting point
2. Hard but brittle
3. Not electrical conductors in solid form
2. Hard but brittle
3. Not electrical conductors in solid form
Characteristics of ionic compounds
A charged group of covalently bonded atoms that result from shortages or excess of electrons
What is a polyatomic ion
Electrons are shared between all the atoms
What is the sea of electrons?
Separation of charge
Pole
polar
Anything that dissolves in water is
Three-dimensional arrangement of a molecule’s atoms
A chemical formula that does not give info on polarity
A chemical formula that does not give info on polarity
What is molecular geometry?
Two atoms always linear
What is a diatomic molecule?
Nonpolar
What does the same electro negativity mean??
1. Hydrogen
2. Nitrogen
3. Oxygen
4. Fluorine
5. Chlorine
6. Bromine
7. Iodine
2. Nitrogen
3. Oxygen
4. Fluorine
5. Chlorine
6. Bromine
7. Iodine
What is the diatomic 7?
Valence-shell electron-pair repulsion
What does VSEPR stand for?
Number of bonded atoms and number of lone pairs on central atom
What is the steric number?
Mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies
What is hybridization?
Orbitals of equal energy produced by the combination of two or more orbitals on the same atom
What are hybrid orbitals?
Hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom
Strongest intermolecular force
Strongest intermolecular force
What is hydrogen bonding?
Forces of attraction between polar molecules
Dipole-dipole
Forcing something that is nonpolar to become polar
A lot weaker
A lot weaker
Induced dipole
Electrical forces that occur because of constant motion electrons
London dispersion forces
Hydrogen: 2
Boron: 6
Phosphorous: 10
Sulfur: 8 or 12
Tenon: 12
Boron: 6
Phosphorous: 10
Sulfur: 8 or 12
Tenon: 12
What are the exceptions to the amount of valence electrons needed when bonded?
The least electronegative
In a Lewis structure, which atom is usually the central atom?
Composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
What is an ionic compound?
Crystalline solids
In what form do most ionic compounds occur?
Ammonium and hydroxide
Give two examples of polyatomic ions
Ionic compounds
In what form do polyatomic ions often occur in nature?
The amount of energy as heat required to vaporize the metal.
How can the strength of metallic bonding be measured?
They’re generally weaker
In general, how do intermolecular forces compare in strength with those in ionic and metallic bonding?
Polar molecules
What type of molecules have the strongest intermolecular forces?
Diatomic molecules’ polarity is determined by one bond but for molecules containing two atoms it’s determined by the polarity and orientation of each bond
What determines the polarity of a molecule?
Nonpolar
Is H-H polar or nonpolar?
Polar
Is H-O polar or nonpolar?
electrons
A chemical bond results from the mutual attraction of the nuclei for
differ in electronegativity
A polar covalent bond is likely to form between two atoms that
one triple bond and one single bond
The Lewis structure of HCN contains
trigonal planar
According to the VSEPR theory, the molecular geometry for CH3+ is
Metallic bonding
An unknown substance is an excellent electrical conductor in the solid state and is malleable. What type of chemical bonding does this substance exhibit?
