en CR Whitney Heagy-Period 3 22 Formula mass: a molecule is the sum of the atomic weights of the atoms in the empirical formula of the compound. Molecular mass: A number equal to the sum of the atomic masses of the atoms in a molecule. The molecular mass gives the mass of a molecule relative to that of the atom, which is taken to have a mass of 12. Avogadroa number: The number of atoms, molecules or particles found in exactly 1 mole of substance. Molar mass: The mass of one mole of a substance, usually expressed in grams or kilograms. Mole: A chemical mass unit, defined to be molecules, atoms, or some other unit. The mass of a mole is the gram formula mass of a substance. Percent composition: percentage by mass of each element in a compound Molecular formula: An expression which states the number and type of atoms present in a molecule of a substance. bond energy: The amount of energy necessary to break one mole of bonds of a given kind (in gas phase). bond length: The equilibrium distance between the nuclei of two groups or atoms that are bonded to each other. coordinate covalent bond: Covalent bond in which both shared electrons are furnished by the same species; bond between a Lewis aced and Lewis base. covalent bond: Chemical bond formed by the sharing of one or more electron pairs between two atoms. double bond: A bond where two electron pairs are shared between two atoms. pi bond: is a covalent bond formed between two neighboring atom’s unbounded p-orbitals. resonance: used to explain properties of the octet rule when a single Lewis structure is inadequate. sigma bond: bonds resulting from the head-on overlap of atomic orbitals, in which the region of electron sharing is along and symmetrical to the imaginary line connecting the bonded atoms. triple bond: is three electron pairs which are shared between two bonded atoms. electron promotion: A statement describing the populations of electronic energy sublevels of an atom. orbital hybridization: Orbital formed by the combination of two or more atomic orbitals. polar covalent bonds: A bond in which a pair of electrons are shared in common between two atoms, but the pair is held more closely by one of the atoms. polyatomic ion: is an ion comprised of two or more atoms. ionic bond: Is a chemical link between two atoms caused by the electrostatic force between oppositely-charged ions in an ionic compound. octet rule: Many representative elements attain at least a share of eight electrons in their valence shells when they form molecular or ionic compounds; there are some limitations.

Whitney Heagy-Period 3

1					2

			3
										4
									5			A

									6			7	N
															8
9								O						10

		11													I
											12
							13					E

				14										U
			15
	16
17			L

						18	I				19

		O
												20
										N
					21										I

						22								T

Across:

5.	a molecule is the sum of the atomic weights of the atoms in the empirical formula of the compound.
6.	is three electron pairs which are shared between two bonded atoms.
9.	A statement describing the populations of electronic energy sublevels of an atom.
12.	The equilibrium distance between the nuclei of two groups or atoms that are bonded to each other.
13.	A chemical mass unit, defined to be molecules, atoms, or some other unit. The mass of a mole is the gram formula mass of a substance.
14.	A bond where two electron pairs are shared between two atoms.

17.	An expression which states the number and type of atoms present in a molecule of a substance.
18.	is a covalent bond formed between two neighboring atom’s unbounded p-orbitals.
19.	bonds resulting from the head-on overlap of atomic orbitals, in which the region of electron sharing is along and symmetrical to the imaginary line connecting the bonded atoms.
20.	The mass of one mole of a substance, usually expressed in grams or kilograms.
21.	The number of atoms, molecules or particles found in exactly 1 mole of substance.
22.	A bond in which a pair of electrons are shared in common between two atoms, but the pair is held more closely by one of the atoms.

Down:

1.	used to explain properties of the octet rule when a single Lewis structure is inadequate.
2.	A number equal to the sum of the atomic masses of the atoms in a molecule. The molecular mass gives the mass of a molecule relative to that of the atom, which is taken to have a mass of 12.
3.	Is a chemical link between two atoms caused by the electrostatic force between oppositely-charged ions in an ionic compound.
4.	Covalent bond in which both shared electrons are furnished by the same species; bond between a Lewis aced and Lewis base.
7.	The amount of energy necessary to break one mole of bonds of a given kind (in gas phase).

8.	Orbital formed by the combination of two or more atomic orbitals.
10.	Many representative elements attain at least a share of eight electrons in their valence shells when they form molecular or ionic compounds; there are some limitations.
11.	percentage by mass of each element in a compound
15.	is an ion comprised of two or more atoms.
16.	Chemical bond formed by the sharing of one or more electron pairs between two atoms.

Whitney Heagy-Period 3

Across:

5.	a molecule is the sum of the atomic weights of the atoms in the empirical formula of the compound.
6.	is three electron pairs which are shared between two bonded atoms.
9.	A statement describing the populations of electronic energy sublevels of an atom.
12.	The equilibrium distance between the nuclei of two groups or atoms that are bonded to each other.
13.	A chemical mass unit, defined to be molecules, atoms, or some other unit. The mass of a mole is the gram formula mass of a substance.
14.	A bond where two electron pairs are shared between two atoms.

17.	An expression which states the number and type of atoms present in a molecule of a substance.
18.	is a covalent bond formed between two neighboring atom’s unbounded p-orbitals.
19.	bonds resulting from the head-on overlap of atomic orbitals, in which the region of electron sharing is along and symmetrical to the imaginary line connecting the bonded atoms.
20.	The mass of one mole of a substance, usually expressed in grams or kilograms.
21.	The number of atoms, molecules or particles found in exactly 1 mole of substance.
22.	A bond in which a pair of electrons are shared in common between two atoms, but the pair is held more closely by one of the atoms.

Down:

1.	used to explain properties of the octet rule when a single Lewis structure is inadequate.
2.	A number equal to the sum of the atomic masses of the atoms in a molecule. The molecular mass gives the mass of a molecule relative to that of the atom, which is taken to have a mass of 12.
3.	Is a chemical link between two atoms caused by the electrostatic force between oppositely-charged ions in an ionic compound.
4.	Covalent bond in which both shared electrons are furnished by the same species; bond between a Lewis aced and Lewis base.
7.	The amount of energy necessary to break one mole of bonds of a given kind (in gas phase).

8.	Orbital formed by the combination of two or more atomic orbitals.
10.	Many representative elements attain at least a share of eight electrons in their valence shells when they form molecular or ionic compounds; there are some limitations.
11.	percentage by mass of each element in a compound
15.	is an ion comprised of two or more atoms.
16.	Chemical bond formed by the sharing of one or more electron pairs between two atoms.