Chapter 6

Question 1

99

Answer 1

Percent of atoms of the human body that come from 4 elements (C, H, N, and O).

Question 2

macronutrients

Answer 2

Elements that are needed in large quantities by your body.

Question 3

trace elements

Answer 3

elements that are needed in very small quantities to maintain optimum health.

Question 4

ionic

Answer 4

A compound formed by the bonding of 1 metal & 1 non-metal as a result of 1 or more electrons being transferred from the metal to the non-metal.

Question 5

molecular

Answer 5

A covalent compound formed by the bonding of 2 or more non-metals as a result of 1 or more electrons being shared (equally or unequally) between the atoms.

Question 6

Mendeleev

Answer 6

The chemist that used density (a physical property) and increasing atomic mass to arrange all known elements into the first periodic table; also recognized many repeating patterns in the ratio of atoms in various compounds.

Question 7

periodic

Answer 7

A term that describes any pattern that repeats at regular intervals.

Question 8

atomic radius

Answer 8

one-half the distance between the nuclei of 2 identical atoms that are bonded together; decreases from left to right across a period and increases down a group or family.

Question 9

electronegativity

Answer 9

The ability of an atom to attract another atom’s electrons when bound to that other atom; increases from left to right across a period and from bottom to the top of a group of elements.

Question 10

ionization

Answer 10

The energy required to remove an electron from an atom; increases from left to right across a period and from the bottom to the top of a group of elements.

Question 11

francium

Answer 11

The last naturally occurring element discovered in 1939; an atomic number of 87.

Question 12

modern periodic table

Answer 12

Arranges elements in order of increasing atomic number and electron configurations.

Question 13

S

Answer 13

Single, spherical orbital that can hold a maximum of 2 electrons.

Question 14

P

Answer 14

Contains 3 dumbbell-shaped orbitals which can hold a maximum of 6 electrons.

Question 15

D

Answer 15

Contains 5 clover-shaped orbitals which can hold a maximum of 10 electrons.

Question 16

F

Answer 16

Contains 7 orbitals of various complex conical and planar nodes which can hold a maximum of 14 electrons.

Question 17

alkali

Answer 17

Soft & extremely reactive Group 1 metals that have 1 electron in their outer energy level; silver, shiny, low density; tend to lose this one electron to become a +1 ion when reacting with a non-metal.

Question 18

alkaline earth

Answer 18

Harder & less reactive Group 2 metallic elements that have 2 electrons in their outer energy level; tend to lose 2 electrons to other non-metals to have a charge of +2.

Question 19

transition metals

Answer 19

The less reactive metals in Groups 3-12 that individually may have various numbers of electrons in the outer energy level and therefore complex bonding properties; most have unfilled d-orbitals.

Question 20

Carbon

Answer 20

An element on the periodic table that is special because it can accept or donate electrons while forming chemical bonds.

Question 21

nitrogen

Answer 21

An element on the periodic table that tends to gain 3 electrons giving it a -3 charge.

Question 22

oxygen

Answer 22

An element on the periodic table that tends to gain 2 electrons giving it a -2charge.

Question 23

halogens

Answer 23

The reactive non-metals in group 7a of the periodic table that contain 7/8 electrons in their outermost energy level; when forming ionic compounds they pull 1 electron away from various metals.

Question 24

noble gases

Answer 24

Inert or unreactive gaseous elements of group 8 on the periodic table; have full outer energy levels preventing them from bonding with other elements.

Question 25

valence

Answer 25

Electrons in the outermost energy level (highest unfilled) of an atom that are the only electrons involved in the formation of ionic or covalent chemical bonds.

Question 26

rule of chemical bonding

Answer 26

Atoms either lose, gain or share valence electrons so that they obtain an electron configuration similar to that of a noble gas.

Question 27

Lewis

Answer 27

A diagram showing one dot for each valence electron an atom has, these dots surround the element symbol of the atom.

Question 28

Ionic Radius Trend

Answer 28

The more + an ion is, the smaller the ionic radius while the more - an ion is, the larger the ionic radius.