Chapter 2 The Structure Of The Atom

Front 1

Dalton Atomic Theory

Back 1

1. Each element t is composed of tiny, indestructible particles called atoms.

2. All atoms of a given element has the same mass and other properties that distinguish them from atoms of other elements.

3. Atoms combine in simple whole number ratios to form molecules of compounds.

4. In a chemical reaction atoms of one element cannot change onto atoms of another element.

Front 2

Rutherford Nuclear Theory

Back 2

1. Most of the atoms mass and it's positive charge are contained in a small core called the nucleus.

2. Most of the volume of the atom is empty space, where negative electrons are dispersed.

3. There are as many negatively charged electrons outside the nucleus as there are protons in the nucleus, so the Atom is neutral.

Front 3

Charge

Back 3

Opposite charges are attracted to each other. Like charges repel

Front 4

Atomic Number

Back 4

The numbers of the protons and it is the letter Z.

Hint 4

Front 5

Isotopes

Back 5

Same element that had atoms with diff masses. The atomic number is the number of protons and the mass number is the protons and neutrons.

Front 6

Charged Atoms

Back 6

Ions: atoms gain or lose electrons, charged particles

Anions: atoms gain electrons, negative charge (nonmetals)

Cations: atoms lose electrons, positive charge (metals)

Front 7

Periodic Law

Back 7

When elements are arranged in order of increasing mass, certain sets of properties occur periodically. In the rows the masses increase from left to right and rows where elements with similar properties fall into the same vertical columns

Front 8

Metals

Back 8

Good conductors of heat and electricity, malleable, ductile, shiny, lose electrons 1A etc..

Front 9

Nonmetals

Back 9

Upper right of periodic table (zigzag between boron to a stating

Solids at room temp, poor conductors of heat and electricity, gain electrons. (Oxygen, carbon, sulfur)

Front 10

Metalloids

Back 10

Lie on the zigzag line

Semiconductors (silicon, arsenic, antimony)

Front 11

Noble gases

Back 11

Group 8A

Unreactive (helium, neon, argon, xenon)

Front 12

Alkali Metals

Back 12

Group 1A

Reactive (Na, Li, K, Rb). Hydrogen is not an alkali. These have low melting points, low density. Li forms red, Na forms yellow, K forms violet for the flame test.

Front 13

Alkaline earth metals

Back 13

Group 2A

Reactive but not compared to alkali. (Calcium, Mg). High melting point and density. CA forms red, Sr forms red, and Ba forms yellow green during flame test. Forms oxides which are unstable which are basic

Front 14

Halogens

Back 14

Group 7A

Reactive nonmetals (chlorine, bromine, iodine, fluorine). Diatomic.