توزيع درجات المقرر (1080 كيم ) final theoretical أعمال فصلية practical...

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( المقرر درجات (1080توزيع كيم

Final Theoretical

فصلية أعمال

Practical Exam

Homework Report Attendance Midterm #2

Midterm #1

40 20 5 10 5 10 10

Time: on Mon., 8:00- 11:00 am, Room: 72Midterm #1: due on week # 7 Midterm #2: due on week # 11Office Hours: Sunday after 11:00, Thursday after 11:00

General Chemistry CHEM 1080

Topics will be covered

• States of Matter• Periodic table• Gases• Liquid• Solids• Chemical Equilibrium• Chemical Kinetics• Solutions

CHAPTER # 1STATES OF MATTER &

PROPERTIES

STATES OF MATTER

Matter is anything that has mass and occupies space.Mass is a measure of the quantity of matter in a sample of any material.

Matter

STATES OF MATTER

solid liquid gas

Solid state

1- Rigid and has definite shapes.

2- Solid is very hard to compress (very slight compressibility).

3- Intermolecular spaces are VERY SMALL

4- Attractive force between atoms is VERY BIG.

5 -Dispersion is VERY SMALL

7- Dispersion is middle.

6- Attractive force between atoms is middle.

5- Intermolecular spaces are middle.

4- Liquids are very hard to compress. (slight compressability)

3- Expansion on Heating is slight.

1- A liquid flows and has the shape of its container.

Liquid state

Gas state

1- Gases are much less dense than liquids and solids.

2- They occupy all parts of any vessel (dispersion is very big)

3- Expansion is infinite.

4- Gases are Very compressible.

5- Intermolecular spaces are Very Big.

6- Attractive force between atoms is very small.

7- Dispersion is Very Big .

PHASE CHANGES

Sublimation is the conversion of a solid directly to a gas without passing through the liquid state; the reverse of that process is called deposition. The changes shown in blue are endothermic (absorb heat); those shown in red are exothermic (release heat). relatively fixed in position, but those in the liquid and gas can flow around each other.

Physical changes that occur among the three states of matter.

A mixture is a combination of two or more substances where there is no reaction.

A. Homogeneous: mixture has uniform properties throughout; like solutions where salts are soluble in solvent

Ex. NaCl + H2O

b- Heterogeneous: a mixture, which is not uniform throughout, substances are insoluble

Ex. Oil + H2O Ex. Sand + H2O

I- Dalton’s Atomic Theory (1808)1. Elements are composed of extremely small particles called

atoms. All atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of one element are different from the atoms of all other elements.

Atoms, Molecules and Ions

2. A molecule is combination of two or more atoms held together by covalent bonds.

H2 H2O NH3 CH4

4. A diatomic molecule contains only two atoms

5. A polyatomic molecule contains more than two atoms.

mass p ~ mass n = 1840 x mass e–

An atom contains equal numbers of electrons and protons.

Atomic number (Z) = number of protons in the nucleus.

Mass number (A) = number of protons + number of neutrons.

XAZMass Number

Atomic NumberElement Symbol

Atom, Atomic number, and Mass number

Atomic NumberElement Symbol

Atomic mass unit (amu), which is defined as exactly 1/12 of the mass atom of carbon -12. atom.

Atomic mass is the mass of an atom in “atomic mass unit” (amu)

By definition: 1 atom 12C “weighs” 12 amu

On this scale

1H = 1.00794 ~ 1 amu

16O = 15.9994 ~ 16 amu

Moles

Defined as a mass in grams equal to atomic mass of a substance contains 6.023 x 1023 particle mol-1

1 mole contains 6.023 x 1023 particles.

6.02 x 1023 is called Avogadro’s number.

One Mole of:

C S

Cu Fe

Hg

3.2

1 mol = NA = 6.023 x 1023

Avogadro’s number (NA)

Mole Calculations

1 mol 12C atoms = 6.023 x 1023 12 C atoms

The mole (mol):

1 mol H2O molecules = 6.023 x 1023 H2O molecules

1 mole NO-3 ions = 6.023 x 1023 NO3

- ions.

Molar mass is the mass of 1 mole of in gramsatoms

1 mole 12C atoms = 6.022 x 1023 atoms = 12.00 g

1 12C atom = 12.00 amu

1 mole 12C atoms = 12.00 g 12C

For any element atomic mass (amu) = molar mass (grams)

Defined as the mass in grams of 1 mole of atoms, ions, or molecules.

Calculate the number of sodium atoms in 0.120 mol Na?

1 mol of Na = 6.022 x 1023 atoms of Na

6.022 x 1023 atoms of Na1 mol of Na

0.120 mol Na X ? atoms of Na

0.120 mol Na x 6.02 x 1023 atoms Na = 7.22 x 1022

1 mol Na

Do You Understand Molar Mass?

Do You Understand Molar Mass?How many atoms are in 0.551 g of potassium (K) ?

1 mol of K = 39.10 g of K

1 mol of K = 6.022 x 1023 atoms of K

0.551 g K

39.10 g K 8.49 x 1021 atoms of K

6.022 x 1023 atoms of K 39.10 g of K

X ? atoms 0.551 g of K

6.022 x 1023 atoms of K =x

Molecular mass (or molecular weight) is the sum ofthe atomic masses (in amu) in a molecule.

SO2

1S 32.07 amu2O + 2 x 16.00 amu SO2 64.07 amu

For any molecule molecular mass in amu = molar mass in grams

1 molecule of SO2 weighs 64.07 amu

1 mole of SO2 weighs 64.07 g

How to calculate molecular mass for a compound

• Ex. H2O

Atomic masses H = 1, O = 16

Molecular mass of H2O = [ 1x2] +16 = 18

One mole of H2O = 18 gram H2O

• Ex. CO2

Atomic masses C = 12, O = 16 Molecular mass of CO2 = 12 +[16 x 2] = 44One mole of CO2 = 44 gram CO2