Drill:

1
Drill

• Calculate the mass in kg of material with a
  density of 7.50 g/mL in a 2.0 m x 500.0 mm x
• 4.00 x 105 mm container.
• 1 cm3 1 mL

2
Chapter 2

• Atoms, Molecules, Ions

3
Atomic Theory

• Elements composed of atoms
• Atoms cant be changed
• Compounds of multiple atoms
• John Dalton

4
Conservation of Mass

• In ordinary chemical reactions, matter can be
  neither created nor destroyed

5
Constant Composition

• Compounds contain elements that are always in the
  same proportions

6
Multiple Proportions

• The elements making up a compound will form whole
  number ratios

7
Atom

• The smallest particle that an element can be
  broken down into and still maintain the
  properties of the element

8
Nuclear Atom

• Proved by Rutherford Bohr in the famous gold
  foil experiments

9
Atomic Composition

• Proton in the nucleus
• Neutron in the nucleus
• Electron outside the nucleus

10
Proton

• In Nucleus
• 1 charge
• About 1 amu in mass

11
Neutron

• In nucleus
• Neutral in charge
• Mass is about 1 amu

12
Electron

• Outside the nucleus
• -1 in charge
• Negligible mass about 1/2000 amu

13
Electron Charge

• Determined by Robert Milliken in the famous oil
  droplet experiment

14
Drill Convert 1) 23 cm/ms to km/ns 2) 56
mg/nL to kg/ML
15
Atomic Number

• The number of protons in an element
• Z number

16
Mass Number

• The number of protons and neutrons in an atom
• A - number

17
Nuclear Symbol

• A 4
• X He
• Z 2

18
Isotopes

• Atoms that contain the same number of protons,
  but different number of neutrons
• Z constant, A variable

19
Atomic Mass

• The weighted average mass of all the isotopes of
  an element
• average of relative abundance x mass number for
  each isotope

20
Periodic Table

• Graphic representation of all the elements
  indicating size, charge, electronic structure,
  reactivity

21
Periods

• Rows which indicate energy level or shell or size
  of the atoms

22
Groups or Families

• Columns which indicate the number of electrons in
  the outermost energy level determining charge
  reactivity

23
Metals

• Left three quarters of the chart
• Lose electrons
• Become positive

24
Nonmetals

• Upper right portion
• Gain, lose, or share electrons when they react

25
Metalloids

• Along the stair-stepped line from B to At
• Share properties of metals nonmetals

26
Radioactivity

• The spontaneous breakdown of an unstable nucleus

27
Radioactive Decay

• Alpha radiation
• Beta radiation
• Gamma radiation

28
Alpha Particle

• Helium nucleus
• 2 protons two neutrons
• mass 4 charge 2
• Low penetrating power

29
Beta Particle

• High speed electron
• Mass 0 charge -1
• Medium penetrating power

30
Gamma Rays

• High energy electromagnetic wave
• No mass or charge
• Very high penetrating power

31
Drill

• List describe each of the three radioactive
  particles

32
Compound

• A group of atoms that are chemically combined

33
Molecule

• A compound that can exist by itself

34
Diatomic Molecule

• Two atoms of the same element that are chemically
  combined
• Cl2, F2, O2

35
Ion

• Charged Particle
• Cl-1

36
Polyatomic Ion

• A group of atoms chemically combined that
  together has a charge
• SO4-2

37
Binary Compound

• A compound made up of two elements in any ratio
• NaCl
• Mg3P2

38
Chemical Formula

• A formula that shows the number and kinds of
  atoms in a compound
• CaCO3

39
Molecular Formula

• A formula that shows the number and kinds of
  atoms in a molecule
• C6H12O6

40
Atomic Structure

• List describe the three subatomic particles

41
Atomic Structure

• Fill in the Chart
• Isotope protons neutrons electrons
• U-235 - - -
• - 56 80 -
• - - 14 13

42
Calculate the atomic mass of the element made up
of the following isotopes99.50 H-10.30
H-20.20 H-3
43
Calculate the atomic mass of the element made up
of the following isotopes5.0 Pu-242, 5.0
Pu-24380.0 Pu-244, 10.0 Pu-245
44
Determine the number of atoms in each compound

• C6H12O6 NaNO3
• H3PO4 Al2(SO4)3