Notes

Unit 3-7 notes pages 172-203

Molecules- group of atoms that are held together by chemical bonds and act as a unit

(Bonds between two or more nonmetals.)

Section 1: Metals

Metals =Good conductors of heat and electricity that reflect light and are solid at room temperature

*Mercury is liquid at room temperature.

(metals are also malleable and ductile)

Malleable =Ability to be hammered or rolled into sheets

Ductile =Ability to be drawn into wires

Metallic Bonding =Positively charged metallic ions are surrounded by a cloud of electrons (the electrons can move freely through the metal)

FAMILIES OF THE PERIODIC TABLE

*Alkali Metals = Group 1A

Group 1 on the periodic table; the most reactive metals that are softer than most other metals

https://www.youtube.com/watch?v=m55kgyApYrY

Radioactive Element =

An element in which the nucleus breaks down and gives off particles and energy

(ex. Francium)

*Alkaline Earth Metals = Group 2A

Group 2 on the periodic table; reactive metals that are not readily found in nature

Transition Elements =

Groups 3 through 12 on the periodic table; made up of metals that can be found in Nature (not as reactive)*D shell

*Lanthanides =

First row of the inner transition metals (named after the element the row follows, Lanthanum) used in motion picture industry F shell

*Actinides =

Second row of the inner transition metals (named after the element the row follows, Actinium) radioactive and unstable F shell

Nonmetals =

Elements that usually are gases or brittle solids at room temperature; NOT malleable or ductile

Diatomic Molecule =

Consists of two atoms of the same element in a covalent bond

(The diatomic molecules are H-NO-Halogens.) H2 = Hydrogen

N2 = Nitrogen

O2 = Oxygen

Br2 = Bromine

Cl2 = Chlorine

F2 = Fluorine

I2 = Iodine

*Halogens = Group 7A

Group 17 on the periodic table; nonmetals (mostly gases) that are very reactive in their elemental form

(ex. Cl2 = chlorine gas)

Salt = (Formed when metals and nonmetals form an ionic bond.)

Term for when a halogen gains an electron from a metal as an ionic bond is formed.

(ex. NaCl = Sodium Chloride)

Sublimation =

Process of a solid changing directly to a vapor without forming a liquid

(ex. dry ice = carbon dioxide solid à carbon dioxide gas)

*Noble Gases =Group 8A

Group 18 on the periodic table; gases that exist as isolated atoms; they are stable and do not react with other elements

(ex. neon, used in lights)

*Inert=

Does not react with other atoms.

Section 3: Mixed Groups

Metalloids =

Can form ionic and covalent bonds with other elements and can have metallic and nonmetallic properties

*Boron Group = Group 3A

Group 13 on the periodic table; a mixed group including metals and a metalloid (boron)

(ex. aluminum, used to make pop cans)

Have 3 valance electrons and have a +3 charge.

*Carbon Group = Group 4A

Group 14 on the periodic table; a mixed group including metals, metalloids, and a nonmetal (carbon)

(ex. silicon, found in sand)

Have 4 valance electrons and have a +/-4 charge.

Allotropes =

Different forms of the same element that have different molecular structures

(ex. carbon allotropes = graphite, diamond, and buckminsterfullerene)

Semiconductors =

Elements that conduct an electric current under certain conditions

(ex. germanium and silicon)

*Nitrogen Group = Group 5A

Group 15 on the periodic table; a mixed group including nonmetals, metalloids, and a metal (bismuth)*These form bonds with a lot of energy!

(ex. nitrogen, used in fertilizers)

*Oxygen Group = Chalcogens =Group 6A

Group 16 on the periodic table; a mixed group including metalloids and nonmetals

(ex. O2 = oxygen gas)

Have 6 valance electrons and have a -2charge.

*Synthetic Elements =

Elements created by smashing existing elements with particles accelerated in a heavy ion accelerator

(ex. technetium 43 and promethium 61)

Transuranium Elements =

Elements that have more than 92 protons (beyond Uranium) these elements are synthetic and unstable

Subscript                                 Name                                                   *Naming covalent compounds*

1                                                          Mono

2                                                         Di

3                                                          Tri

4                                                          Tetra

5                                                          Penta

6                                                          Hexa

7                                                          Hepta

8                                                          Octa

9                                                          Nona

10                                                       Deca

Naming covalently bonded compounds.

1. List the prefix that indicates the subscript of the first element.

2. Write the name of the first element.

3. List the prefix that indicates the subscript of the second element.

4. Write the name of the second element with the -ide ending.

Ex.

C5Cl8

Pentacarbon Octachloride

Calculating the mass of the compounds:

Atom                 subscript X average mass=total mass

Carbon             5  X 12  =  60 g/mol

Chlorine           8 X 35.5=284 g/mol

                             Total=344 g/mol

Metals usually possess the following characteristics:

1. Malleable: Able to be pounded into various shapes and NOT lose strength.

2. Ductility: Able to be drawn into a wire.

3. Luster: Reflect light/ shiny appearance.

4. Conductor: Able to transmit electricity and heat very readily.

5. Reactivity: Produce hydrogen gas when mixed with acids (oxidize (rust) in the presence of CuCl2 [copper(ll)chloride].)

Nonmetals usually possess the following characteristics:

1. Brittle: Break when hit with a hammer.

2. Dull: Most do NOT reflect light nor appear shiny.

3. No ductility: Can NOT be drawn into a wire.

4. Nonconductor: Do NOT transmit heat or electricity.

5. Reactivity: Do NOT react with acid to form H2 gas or oxidize in CuCl2 [cupric chloride].

•          CALCULATE THE % MASS FOR EACH ELEMENT

A)  Ca (NO3)2

Ca=>1*40 =40  40/ 164 X 100 =24%

N=>2*14= 28   28/164 = X 100 17%

O=>6*16=96  96/164= X 100 59%

Total Mass =40+28+96= 164 g/mol

B)  C2N4O

   C=>2*12 =24   24/ 96 X 100 =25%

  N=>4*14= 56   56/96 X 100 =58%

  O=>1*16=16  16/ 96 X 100 =17%

  Total Mass =24+56+16= 96 g/mol