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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.

Published byGwenda Gardner Modified over 6 years ago

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Presentation on theme: "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."— Presentation transcript:

1 Drill: Calculate the mass in kg of material with a density of 7.50 g/mL in a 2.0 m x 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 can’t 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 Proved by Rutherford & Bohr in the famous gold foil experiments
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 Determined by Robert Milliken in the famous oil droplet experiment
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 X He Z

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 Rows which indicate energy level or shell or size of the atoms
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 List & describe each of the three radioactive particles
Drill: List & describe each of the three radioactive particles

32 A group of atoms that are chemically combined
Compound A group of atoms that are chemically combined

33 Molecule A compound that can exist by itself

34 Two atoms of the same element that are chemically combined
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 List & describe the three subatomic particles
Atomic Structure List & describe the three subatomic particles

41 Atomic Structure Fill in the Chart: Isotope protons neutrons electrons

42 Calculate the atomic mass of the element made up of the following isotopes: % H % H % H-3

43 Calculate the atomic mass of the element made up of the following isotopes: 5.0 % Pu-242, 5.0 % Pu % Pu-244, & % Pu-245

44 Determine the number of atoms in each compound
C6H12O6 NaNO3 H3PO4 Al2(SO4)3

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