I have learned about: Scientific notation significant figures metric system classification of matter physical properties of matter chemical properties of matter phases of matter

I have learned about: Law of conservation of mass Periodic Table Basics Temperature Heat Specific Heat Heat Equation

I have learned about: Ions Isotopes Average atomic mass Atoms (protons, neutrons, e-) Ions Isotopes Average atomic mass e- configurations ground state excited state Bright line spectra

Significant Figures 1 2 11 10 100 1000 1000. One sig fig Two sig figs four sig figs

Significant Figures 1200 1200. 1263 1207 two sig figs four sig figs

Significant Figures 0.1 0.01 0.0004 0.203 0.62397 0.00694 one sig fig three sig figs five sig figs

Significant Figures 56.2 56.007 56.0 56 50.00 3 5 2 4

Sig Figs in Scientific Notation 5.347 x 10 16 5.347 4 sig figs 5.000 x 10 -6 5.000 4 sig figs 5 x 10 -6 5 1 sig fig

Multiplying with Sig Figs

Adding with Sig Figs

Classification of Matter

States of Matter GAS LIQUID SOLID

Physical Properties of Matter The properties of a substance that can be demonstrated without changing the composition of the substance Size (length, volume) Density Mass Color

Ex. Water boils into steam at 100 degrees Celsius Physical Properties Melting Point Ex. Ice (solid water) starts to melt to liquid water at 0 degrees Celsius Boiling Point Ex. Water boils into steam at 100 degrees Celsius

Malleability: can be pounded into a new shape without breaking Physical Properties Malleability: can be pounded into a new shape without breaking Metals are malleable

Physical Properties Iron is malleable Fe

Can be pulled into long wires without breaking Physical Properties Ductility Can be pulled into long wires without breaking Metals are ductile

Reflects the regular arrangement of atoms in the solid Physical Properties Crystal Shape Reflects the regular arrangement of atoms in the solid

Physical Change A change in the sample of matter that does not result in a NEW substance: Phase Changes Changes in shape Solid liquid gas

Chemical Properties of Matter How matter behaves when it changes into a NEW substance. EX. Iron rusts silver tarnishes Milk sours sugar ferments eggs rot leaves turn paper burns

Substance changes into a NEW substance. Chemical Change Substance changes into a NEW substance. This change is often an irreversible and permanent change in composition

Burning

Tarnishing

Rusting

Oxidizing

Chemical changes mean a chemical reaction has occurred REACTANTS PRODUCTS old substances become new substances Sodium + Chlorine sodium chloride (table salt) Na + CL NaCL

Classify the following samples:

Classify the particles of matter

Identify the following changes as Physical or Chemical

Identify the following changes as Physical or Chemical Fe

Identify the following changes as Physical or Chemical

Periodic Table Review Elements are arranged according to______ Vertical columns are called________ Horizontal rows are called ________ There are ______ periods in the table Most elements are classified as _____ Where are the transition metals? What are the metalloids?

Units of Energy Energy is measured in JOULES Also in calories or kilocalories (food) How many calories are in a kilocalorie?

High temperature = moving faster What is temperature? A measure of the average kinetic energy of the particles in a sample of matter. All atoms are moving! High temperature = moving faster

AVERAGE KINETIC ENERGY Once again…… TEMPERATURE = AVERAGE KINETIC ENERGY

Kelvin never goes below zero (no negative numbers!) Temperature Scales Kelvin: 0 K = absolute zero (-460 oF) all motion of particles stops! Water freezes @ 273 K Water boils @ 373 K Kelvin never goes below zero (no negative numbers!)

Temperature Scales Kelvin = Celsius + 273 Celsius = Kelvin – 273 If it is 32O Celsius, what temperature is it in Kelvin? If it is 100 Kelvin, what temperature is it in Celsius?

What is Heat? Heat is the sum total of all the kinetic energy in a sample of matter. How is heat different from temperature???

Heat ≠ Temperature Both the water in the bath tub and in the cup are at 25 oC Which contains more HEAT?

Specific Heat Capacity The amount of energy (in JOULES) needed to raise the temperature of 1 gram of the sample by 1 oC Which water sample has a higher specific heat ?

HEAT EQUATION (in Table T) Q = mc∆t Q = heat energy in JOULES (J) m = mass of the sample in GRAMS (g) C = specific heat in J/goC ∆t = change in temperature (oC) or final temp – initial temp

Ion An atom that has gained an electron is called an anion. It has a net negative charge. An atom that has lost an electron is called a cation. It has a net positive charge.

do they have different atomic masses? Isotope Atoms of the same element that have different atomic masses (but same atomic number) WHY do they have different atomic masses?

Isotope If two atoms are of same element, they MUST have the same number of protons (the same atomic number) But…. they can have different number of NEUTRONS. The more neutrons, the heavier the atom

Isotopes of Lithium 3 neutrons 5 neutrons 4 neutrons

Average Atomic Mass In nature, most elements are a mixture of different isotopes The mass of a sample of an element is a weighted average of all the isotopes in the sample

Calculating Average Atomic Mass The element Chlorine Cl has two naturally occurring isotopes: Cl-35 and Cl-37 Which isotope has more neutrons? How many more neutrons?

Calculating Average Atomic Mass Out of 100 chlorine atoms, 75 will have a mass of 35 amu. 25 will have a mass of 37 amu

Calculating Average Atomic Mass If 75% of all chlorine atoms in nature are Cl-35 and 25 % are Cl-37, what is the average atomic mass of a sample of chlorine? *** Remember, this is a weighted average!

Calculating Average Atomic Mass The unweighted average of 35 and 37 is… 36 This is NOT our answer!

Calculating Average Atomic Mass The weighted average is calculated using the following formula (memorize this!) (mass of isotope A x %) + (mass isotope B x %) 100

Calculating Average Atomic Mass (mass of isotope A x %) + (mass isotope B x %) 100 (35 amu x 75) + (37 amu x 25) = 100 35.5 amu

Atom Review 3. What is located in the nucleus of the atom? 4. What is the nuclear charge (the charge on an atom’s nucleus)? 5. Where in the atoms are e- found? 6. What is the atom mostly made of?

Atom Review For each of the subatomic particles, give Mass Charge Location Proton Neutron electron

Atom review What is an ion? Name the 2 kinds of ions What is an isotope?

Atom Review 11. What information does the atomic number of an element tell you? What 2 subatomic particles give the atom most of it’s mass? What does AMU stand for and what atom is it based on?

Atom Review 14. Write the formula we use to find the average atomic mass of an element:

Atom Review Questions Neutral atoms contain equal numbers of All isotopes of neutral sodium atoms contain _________ protons and ___________ electrons

Atom Review Questions Hydrogen has 3 isotopes. For each one tell how many protons, neutrons and e- H-1 H-2 H-3

Atom Review Questions 4. For each isotope of oxygen tell how many protons, neutrons and e- O-16 O-17 O-18

Atom Review Questions What is the charge on an atom that contains 9P, 10N, 9e-? What is this atom’s atomic number? What is its atomic mass?

Atom Review Questions Cl-35 contains ______protons ______ neutrons ______ electrons

Atom Review Questions For the atoms below, list the number of protons, neutrons, and electrons Kr 84 36

Atom Review Questions For the atoms below, list the number of protons, neutrons, and electrons Cu +2 64 29

Atom Review Questions For the atoms below, list the number of protons, neutrons, and electrons F -1 19 9

Atom Review Questions For the atoms below, list the number of protons, neutrons, and electrons P -3 31 15

Atomic Review Questions Write an isotope of O Write an ion of O 16 8 16 8

Atomic Review Questions 12. Describe Rutherfords Gold Foil Experiment 13. What were the 2 conclusions about the structure of the atom that resulted from the Gold Foil Experiment? 16 8 16 8

Excited State e- Ground State

For an e- to jump from the ground state to the excited state, it must absorb energy (a photon of light) When an e- falls back down from excited state to ground state, it releases energy (a photon of light)

The visible light produced by e- falling back to ground state is called a bright line spectrum Light is emitted only at certain wavelengths

Each element has its own distinct bright line spectrum Bright line spectra can be used to identify elements, by comparing the spectral lines to known spectra

To Summarize: 7 energy levels 4 sublevels ( S, P, D, F) S orbitals = holds 2 e- P orbitals = holds 6 e- D orbitals = holds 10 e- F orbitals = holds 14 e-

Arrangement of e- in the atom 7 s 7 p 7 d 7 f 6 s 6 p 6 d 6 f 5 s 5 p 5 d 5 f 4 s 4 p 4 d 4 f 3 s 3 p 3 d 2 s 2 p 1 s

Electron configuration for Ne ___ ___ ____ ____ ____ 1s 2s 2p 2 2 6

Write the e- configuration of As 33

Write the e- configuration of As 33 ___ ___ ___ ___ ___ ___ ___ ___ ___ 1s2 2s2 2p6 3s2 3p6 ___ ___ ___ ___ ___ ___ ___ ___ ___ 4s2 3d10 4p3 e- will not pair up in p, d or f orbitals if there is room in the orbital for them to spread out !

1s2 2s2 2p6 3s2 3p6 4s2 2 – 8 - 8- 2

What element? 5 2 2

What element? 2 2 6 2 3