Question

Definitions. Fill in the blank with the LETTER of the most appropriate term from the following:
A. metal                                B. principal quantum number, n
C. metalloid                           D. non-metal
E. ionic bond                          F. azimuthal quantum number, l
G. covalent bond                       H. magnetic quantum number, ml
I. ionization energy                   J. atomic size
K. polyatomic ion                       L. Lewis structure
M. Bohr                                 N. Mendeleev
O. polar bond                          P. octet rule
R. electronegativity                   S. valence shell
T. ion                                 V. periodic table

_________ determines the shape of an atomic orbital

_________ electrons in outermost energy level that may bond with other atoms

_________ determines the distance of the electron from the nucleus

_________ measures the tendency of an atom to lose one electron and become a +1 ion

_________ systematic arrangement of the elements in order of increasing atomic number

_________ atoms tend to seek the configuration of a noble gas in valence shell

_________ created when an atom either gains or loses electrons

_________tend to gain electrons and have negative oxidation numbers in compounds

_________ credited with the organization of modern periodic table

_________ tendency of an atom to pull electrons toward itself in a covalent bond

_________tend to lose electrons and become positively charged ions

_________formed when a metal atom and a non-metal bond by gain and loss of electrons

_________ developed first model of atomic structure based on energy levels

_________ two atoms with different electronegativity values create a separation of electron density

_________ group of two or more atoms which are covalently bonded an act as a single ion

_________ formed when two atoms share electrons

_________dot diagrams showing electrons in atom’s valence shell

___________ determines the number of orbitals within a subshell by its values from –l to +l

___________ decreases across a period (from left to right)

___________ can gain or lose electrons in a bond

Answer 1

ANSWERS

1) Azimuthal quantum number, l determines the shape of an atomic orbital.

2) Valence shell electrons in outermost energy level that may bond with other atoms.

3) Principal quantum number, n determines the distance of the electron from the nucleus.

4) Ionization energy measures the tendency of an atom to lose one electron and become a +1 ion.

5) Periodic table systematic arrangement of the elements in order of increasing atomic number.

6) Octet rule atoms tend to seek the configuration of a noble gas in valence shell.

7) Ion created when an atom either gains or loses electrons.

8) Non-metals tend to gain electrons and have negative oxidation numbers in compounds.

9) Mendeleev credited with the organization of modern periodic table.

10) Electronegativity tendency of an atom to pull electrons toward itself in a covalent bond.

11) Metals tend to lose electrons and become positively charged ions.

12) Ionic bond formed when a metal atom and a non-metal bond by gain and loss of electrons.

13) Bohr developed first model of atomic structure based on energy levels.

14) Polar bond two atoms with different electronegativity values create a separation of electron density.

15) Polyatomic ion group of two or more atoms which are covalently bonded an act as a single ion.

16) Covalent bond formed when two atoms share electrons.

17) Lewis structure dot diagrams showing electrons in atom’s valence shell.

18) Magnetic Quantum number determines the number of orbitals within a subshell by its values from –l to +l.

19) Atomic size decreases across a period (from left to right).

20) Metalloid can gain or lose electrons in a bond.