Chapter 6 Electronic Structure and Chemical Periodicity

Question 1

Periodic Law

Answer 1

When elements are arranged in order of increasing atomic number, elements with similar chemical behavior occur ar periodic intervals

Question 2

Period

Answer 2

Horizontal row of elements in the periodic table

Question 3

Group

Answer 3

vertical column of elements in the periodic table

Question 4

Alkali Metal

Answer 4

General name for any element in the IA group of the periodic table excluding hydrogen. Soft shiny. React well with water

Question 5

Alkaline Earth Metal

Answer 5

general name for any element in the IIA group. Soft and shiny. Only moderately reactive with water.

Question 6

Halogen

Answer 6

Group VIIA. Very reactive colored substances that are gases at room temperature

Question 7

Noble Gas

Answer 7

Group VIIIA. Unreactive gases. Undergo few chemical reactions if any

Question 8

Quantized Property

Answer 8

property that can only have certain values. Only certain values allowed.

Question 9

Electron Shell

Answer 9

region of space about a nucleus that contains electrons that have approximately the same energy and spend most of their time approximately the same distance from the nucleus

Question 10

Electron Subshell

Answer 10

region of space within an electron shell taht contains electrons that have the same energy

Question 11

Order of Subshells

Answer 11

S P D F (energy increases from S to F)

Question 12

Electron Orbital

Answer 12

region of space within an electron subshell where an electron with a specific energy is most likely to be found

Question 13

Characteristics of Electron Orbitals

Answer 13

1) The number of orbitals in a subshell varies, being one for an S shell, 3 for a P shell, five for a D shell, and seven for an F shell
2) The max number of an electrons does not vary. It is always two
3) The notation used to designate orbitals is the same as that used for sub shells. Thus orbitals in the 4F sub shell (7) are all called 4f sub shells

Question 14

Electron Spin

Answer 14

property of an electron associated with the concept that an electron is spinning on its own axis.

Question 15

Electron Configuration

Answer 15

statement of how many electrons has in each of its sub shells. Consists of a number for the shell followed by a letter for the sub shell plus a superscript number indicating how many electrons are in that shell

Question 16

Aufbau Diagram

Answer 16

listing of electron sub shells in the order in which electrons occupy them

Question 17

Condensed Electron Configuration

Answer 17

electron configuration in which the chemical symbol of the nearest noble gas element of the lower atomic number used to represent the electrons in the configuration up to that noble gas, and the remaining additional electrons are then appended to the chemical symbol of the noble gas.

Question 18

Core Electrons

Answer 18

inner shell electrons of an atom that are not normally involved in determining the chemical properties of the atom.

Question 19

Outer Electrons

Answer 19

electrons in the condensed notation after the noble gas

Question 20

Hund’s Rule

Answer 20

when electrons are placed in a set of orbitals of equal energy (the orbitals of a sub shell), the order of filling for the orbitals is such that each orbital of the subshell receives an electron with the same spin before any orbital receives a second electron of the opposite spin

Question 21

Paired Electrns

Answer 21

two electrons of opposite spin in the same orbital

Question 22

Unpaired Electron

Answer 22

single electron in an orbital

Question 23

Paramagnetic Atom

Answer 23

atom that has an electron arrangement containing one or more unpaired electrons

Question 24

Diamagnetic Atom

Answer 24

an atom that has an electron arrangement in which all electrons are paired.

Question 25

Distinguishing Electron

Answer 25

last electron added to the elements configuration when the configuration is written according to the aufbau principle

Question 26

Writing Electron Configurations Using the Periodic Table

Answer 26

1) Begin with hydrogen and helium
2) Continue through the elements in other periods, in order of increasing atomic number
3) As you move across a period:
a. add electrons to the ns sub shell as you pass through the s area.
b. add electrons to the np sub shell as you pass through the p area
c. add electrons to the (n-1)d sub shell as you pass through the d area.
d. add electrons to the (n-2)f sub shell as you pass through the f area
4) Continue until you reach an element whose electron configuration you are writing.

Question 27

Metal

Answer 27

an element that has the characteristic properties of luster, thermal conductivity, electrical conductivity, and malleability.

Question 28

Nonmetal

Answer 28

an element characterized by the absence of luster, thermal conductivity, electrical conductivity, and malleability

Question 29

Representative Element

Answer 29

an element located in the s area or the first five columns of the p area.(the p area minus the noble gases)

Question 30

Transition Element

Answer 30

Elements located in the d area. All are metals

Question 31

Inner-transitional Elements

Answer 31

Located in the f area.

Question 32

Chemical Periodicity

Answer 32

variation in properties of elements as a function of their position in the periodic table.

Question 33

Metalloid

Answer 33

an element with properties in between metals and nonmetals

Question 34

Semiconductor

Answer 34

element that does not conduct electricity at room temperature but does at higher temperatures.