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What is a chemical bond?
Mutual electrical attraction between the nuclei & valence electrons of different atoms.
Explain the difference between ionic and covalent bonds in terms of electrons.
Covalent bonds share electrons --- In ionic bonds, electrons are attracted to the nucleus of another.
How does a polar covalent bond differ from a non-polar covalent bond?
Polar--> unequal sharing of electrons Non-Polar---> equal electron sharing
Define "molecule"
Neutral group of covalently bonded atoms.
What is a molecular formula?
Type and number of atoms needed to make a molecule.
Longer bonds tend to be ___________ than shorter bonds.
Weaker
How many valence electrons do atoms seek to achieve?
8
Define an ionic compound.
Postitive and negative ions that have a net charge of zero.
What is an anion?
A negative ion
What is a cation?
A positive ion
What is the difference between a covalently bonded "molecule" and an ionicly bonded "crystal" in terms of atoms?
Ionic-lowest ratio Covalent- exact #
How do covalent and ionic bonded substances differ in properties?
Covalent-->low melting point, don't conduct electricity, don't dissolve in water Ionic--->high melting point, conduct electricity, dissolve in water
Ammonia is polar because its shape is _____________.
Pyramidal
What are the 3 types of bond?
Covalent, Ionic, & Metallic.
What is the difference between polar and non-polar bonding?
Polar---> unequal sharing of electrons Non-Polar---> equal sharing
If the difference in electronegativity is between two atoms is less that 1.0 it is (1), if the difference in electronegativities is greater than 1.7 it is (2) , & if the difference is between 1.0 & 1.7 it is (3)_.
Non-Polar Covalent
Ionic
Polar Covalent
When electrons are shared between atoms, are the electrons in a higher or lower energy state than when they are in separate atoms?
Lower
What is a molecule?
Covalently bonded atoms.
A _________________ shows the number & type of atoms in a molecule.
Molecular Formula
The attraction between the (1)_ of one atom and the (2)_ of another atom cause the potential energy to be at its lowest and a bond to form.
Nucleus
Electrons
Define "bond length".
The average distance between 2 atoms.
Define "bond energy". What compounds are more stable: ones with high bond energy or ones with low bond energy.
Bond energy is energy required to break a bond. Compounds with high bond energy are more stable.
As bond length increases the bond energy ____________.
Weakens
Shorter bonds are __________ than longer bonds.
Stronger
State the octet rule.
All atoms want 8 valence electrons.
What is an unshared pair of electrons?
Unbonded pairs of electrons on the center atom.
Write the formula unit for the ionic compound formed by Ca2+ and Br-
CaBr2
What kind of structure do we find ionic compounds in?
Crystals
Explain the metallic bond.
Attraction between metal atoms and surrounding electrons.
List some properties of metals.
Free electrons, ductile, malleable.
What is an intramolecular force?
Forces of attraction between molecules.
What are the three types of intramolecular forces? List them in order from strongest to weakest.
Dipole-Dipole, Hydrogen, London Dispersion (Van Der Waals)
Which intramolecular force holds non-polar molecules together?
London Dispersion (Van Der Waals)
Word to describe a molecule with an unequal charge distribution.
Dipole
Type of bond formed between an active metal and a nonmetal.
Ionic
The simultaneous attraction of electrons for the nuclei of two or more atoms is a chemical ______________.
Bond
Bonding that is responsible for the relatively high boiling point of water.
Ionic
Type of covalent bond found in diatomic molecules,
Nonpolar
Particles formed from covalent bonding.
Molecules
Compounds with both ionic and covalent bonds contain this type of ion.
Polyatomic
Type of bond found in aluminum foil
Metallic
The formulas of ionic compounds must be expressed as ____________ formulas.
Empirical
The shape of a water molecule.
Bent
Type of bond found between nonmetals.
Covalent
Type of covalent bonding that is found in the diamond.
Network
Type of covalent bond found between atoms of different electronegativity values.
Polar
Force of attractive between nonpolar molecules.
Van Der Waals
Element with the highest electronegativity value.
Fluorine
