Chemistry (5/8)Due Today:•Stoichiometry Worksheet•Gas Laws Graphs

Objectives:•Complete Stoichiometry Quiz • Interpret and discuss the Gas Laws graphs by answering the questions in your packet.

Chemistry (5/9)Due Today:•Stoichiometry Worksheet-late•Gas Laws Graphs

Objectives:• Discuss the Gas Laws you read about from the text and applied to graphs. •Discuss Stoichiometry Quiz

Homework:

Study for Stoichiometry Re-Take Quiz

Gas Laws AssignmentChapter 14.2 in Text

•Graph each set of data using a line graph.

•Interpret each graph by answering the questions in the packet.

Gas Laws

Behavior of a gas when two of the following variables change:

• temperature of a gas (oC or K)• pressure of a gas (atm, mmHg, Pa)• volume of a gas ( mL, cm3)

Illustrate in your notes how a sample of gas in a balloon would be affected by a change in each variable above.

Gas Laws1. Volume vs. Pressure Graph

Boyle’s LawIf temperature is held constant, what is the relationship between the volume and pressure of a gas?

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Gas Laws2. Temperature vs. Volume Graph

Charles’ Law

If pressure is held constant, what is the relationship between temperature and volume of a gas?

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Gas Laws3. Temperature vs. Pressure of a Gas

Gay-Lussac’s Law

If volume is held constant, what is therelationship between temperature and pressure?

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Combined Gas Law• Establishes a relationship between pressure,

volume, and temperature of a gas if the amount of gas is held constant.

• P1V1/T1= P2V2/T2

Ideal Gas Law• Establishes a relationship between pressure,

volume, temperature, and quantity of a gas. • PV=nRT,where P= pressure (atm)• V= volume (Liters)• n= quantity of gas (moles)• R= gas constant: 0.0821 L-atm/mol-K• T= temperature (Kelvin)

Chemistry Introduction:Measurement and Scientific Method

Measurement and Scientific Method:Precision vs. Accuracy

Label each picture as precise, accurate, both, or neither.

Matter and Change

Phase Changes and Kinetic Energy

Atomic Structure

Electromagnetic Spectrum

Bohr’s Model of the Atom

• The electron cloud consists of energy levels.

• Electrons reside and move around in these energy levels.

• Electrons can move to other energy levels when absorb photons.

Electron Movement

1.Ground state of H Atom (lowest energy level for e-)2.A photon (light particle) is absorbed by H’s electron. Electron becomes excited and jumps to higher energy

level.3. E- returns to ground state and emits (releases) the

photon.

Emitted photon’s wavelength can be detected by scientists.

(Infrared region at room temp; Visble region at higher temps.)

1. 2. 3.

Electron Properties and Arrangement

Electron Properties and Arrangement

Electron Properties and Arrangement

Periodic Table

Periodic Table:Atomic Radius

Periodic Table:Ionization Energy

Chemical Bonding

Chemical Reactions

Types of Chemical Reactions1. Synthesis (A+ B ----> AB)

2. Decomposition (AB------> A + B)

3. Single Replacement (A+ BC ---> B + AC)

4. Double Replacement (AB + CD ---> CB + AD)

5. Combustion (CxHx + O2 ----> CO2 + H2O)

6. Neutralization (Acid + Base--> H2O + Salt)

Chemical Reaction Energy Diagram:Exothermic

Chemical Reaction Energy DiagramEndothermic

Chemical Reactions Rates• Reaction Rates = how fast the reactants

chemically change into the products. • Collision Theory: Reactant particles will

form products when reactants collide:- at the right position.- and exchange the right amount of kinetic

energy.

Nuclear Chemistry

Nuclear Band of Stability

http://www.hasdeu.bz.edu.ro/softuri/fizica/mariana/Atomica/Table/lessons/11nuclear/nuclear.htm

*Big Misconception: Stable nucleus means equal number of protons and neutrons. From graph, students confirmed that most elements with a stable nucleus needs more neutrons to minimize the repulsion force between protons with a similar charge.

Nuclear Chemistry:Radioactive Decay

Chemical Quantities

number ofrepresentative

particles

mass

1 mol22.4L

22.4L1 mol

6.02 x 10 particles1 mol

23

6.02 x 10 particles231 mol

1 molmolar mass

molar mass1 mol

moles

volumeat STP

Stoichiometry

Chemistry Final

What does Chemistry study?

Scientific Notation

1. Convert to scientific notation:

2,350,921

Scientific Notation

• Convert to scientific notation .

0.0000258

Metric Conversion

Kilo-, Hecto-, Deka-, Base, Deci- Centi-, Milli-

• 5 kg = ________cg

Metric Conversion

Kilo-, Hecto-, Deka-, Base, Deci- Centi-, Milli-

• 3.5cL= ______ L

Metric and English Conversions

How many seconds is in 10.26hrs?

Metric and English Conversions

• Sara ran 2 miles in 16 minutes. How far did she run in kilometers? (1mi= 1600m)

Density

What is the equation for density?

Density

• A solution has a mass of 1200 g and a density of 1.2 g/mL. What is the volume?

Density

• What is the density of a 50mL sample of water that has a mass of 49.6 g?

Scientific Method

• What are the 5 main steps to the scientific method?

Scientific Method

What is the difference between qualitative and quantitative results?

Scientific Method

• What is the difference between accuracy and precision?

Scientific Method

• Determine which of the following sets of data is most precise.

a. 2.5, 6.0, 4.0

b. 2.5, 3.0, 2.0

c. 2.5, 2.4, 2.3

Scientific Method

• A student wanted to know how temperature affected the rate of a chemical reaction. She observed and recorded the time it took for a chemical reaction to occur at three different temperatures.

What is the independent variable?

What is the dependent variable?

Significant Figures

• How many significant figures?

0.01020g ________

Significant Figures

• How many signficant figures?

• 2.104_______

Calculating using Significant Figures

• How many significant figures are in the answer?

1.21 g x 0.50g =

Calculating using Signficant Figures

• How many significant figures are in the answer?

0.45m + 2.140m + 1.3g+ 4g =

Matter

• What are the two broad classes of matter?

Classification of Matter

Matter

• What is the big difference between substances and mixtures?

Mixtures

• Determine if the following mixtures are heterogenous or homogenous mixtures.

a. Saltwater

b. Vegetable soup

Compounds

True or False: Compounds composition is always varied.

True or False: A compound’s properties are similar to the elements making up the compound.

Physical Properties

Give me example of physical properties.

Chemical properties

Give me example of chemical properties.

Physical or Chemical Change

• Determine if the following are chemical or physical changes

a. Boiling water

b. Digesting food

c. Burning fire wood

d. Dissolving sugar in water

Mixture or Compound?

• air

• Na(OH)

• lead

• Na(OH)solution

Atomic Theory

• Who believed matter consisted of air, wind, fire, and earth?

• Who was the first to propose that matter is composed of atoms?

Atomic Theory

• Who was the first person to confirm using the scientific method that matter was composed of atoms?

Dalton’s Atomic Theory

• Identify important concepts of Dalton’s Atomic Theory.

The Atom

• What are the two subatomic particles that have charge?

The Atom

• What are the two subatomic particles that contribute mass to an atom?

The Atom

• What is the difference between mass number and atomic mass?

Atomic Subparticles• Nitrogen is a neutral atom. It has 7neutrons and

7 electrons.

• What is Nitrogen’s number of protons?

• What is Nitrogen’s atomic number?

• What is Nitrogen’s mass number?

Atomic Subparticles

• Ca 2+ has a mass number of 40 and an atomic number of 20.

• How may protons does Ca 2+ have?

• How many electrons does Ca 2+ have?

• How many neutrons does Ca 2+ have?

The Atom

• What is an isotope?

Bell Ringer

• How many significant figures?

a. 0.040020____

b. 1.0200_____

c. 10,840______

d. 24.09/ 4.2______

e. 4.25 + 4.0 = ______

Isotope

• C-12 and C-13 are isotopes.

What subatomic particle has the same value with each isotope of carbon above?

What subatomic particle has different values with each isotope of carbon above?

Radioisotope

• What is a radioisotope?

• What are the three types of radioisotope particles we talked about?

Nuclear Radiation

paper

wood

concrete or lead

Radiation charges Radiation Penetration

Alpha ParticlesAlpha rays(α) = Emission of a He nucleus. • alpha particles are (+) charged .• large mass and charge prevents alpha particles from

traveling and penetrating far.

1.

parent decays α + daughter isotopeisotope particle (stable) (unstable) (He nucleus)

Nuclear Decay with α Particles

• Mass number decreases by four

• Atomic Number decreases by two

(Daughter isotope that is more stable)

Nuclear Decay: Beta Particles• Beta Rays (β) = A neutron breaks into a p+

and e-• p+ remains in nucleus and e- is emitted.• Beta rays have a (-) charge.• Beta rays travel and penetrate farther

because smaller charge and no mass.

Nuclear Decay with β particles

• Mass number remains the same

(proton switches with a neutron)

• Atomic number increases by one.

(proton formed in nucleus; stable daughter isotope).

Nuclear Decay: GammaGamma Rays(ϒ) = high energy particle with no mass or charge.Does not have a charge or mass, therefore travels and penetrates the farthest.Most dangerous rays because penetrates skin.Usually emitted with alpha and beta particles.

parent decays α + daughter isotope + ϒ

isotope particle (stable) (unstable) (He nucleus)

+ϒ

Nuclear Decay with ϒ rays

• Mass number remains the same

(ϒ rays has no mass)

• Atomic number remains the same

(ϒ rays has no mass or charge)

Periodic Table

• Who organized the periodic table based on atomic mass?

Periodic Table

• Who organized the periodic table based on atomic number?

Periodic Table

• How is the modern periodic table

Organized?

Periodic Table

• What is another name for rows on the periodic table?

Periodic Table

• What is another name for the columns on the periodic table?

Periodic Table

• Give me an example of a metal, non-metal, and a metalloid

Periodic Table

• What is the difference between transitional and representative groups?