Presentation_SAT II Chem_bonding

Course Calendar : Course Calendar SAT II PREP

Course Calendar : Course Calendar SAT II PREP

Course Calendar : Course Calendar SAT II PREP

Topics Covered : Topics Covered SAT II PREP Structure of Matter 25% Atomic structure ? Molecular structure ? Bonding ? States of matter 16% Gases ? Liquids & solids ? Solutions ? Reaction types 14% Acids & bases ? Oxidation-reduction ? Precipitation ? Stoichiometry 14% Molec concept ? Chemical equations ? Equilibrium & Reaction rates 5% Equilibrium systems ? Rates of reactions ? Thermochemistry ? 6% Descriptive chemistry ? 12% Laboratory ? 8%

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Key terms Subatomic particles Neutron Proton Electron Mass # Atomic # Line emission spectra Isotope Ions Electronic configuration Bohr model of atom Quantum mechanical model Principal quantum number Angular momentum quantum number Azimuthal quantum number Magnetic quantum number Spin quantum number Ground state Excited state s-orbital p-orbital d-orbital Nucleus Subshell Heisenberg uncertainty principle Pauli exclusion principle Atomic mass unit Atomic weight Quantization Rutherford Thomson Cathode ray tube Gold foil experiment Energy level

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Key concepts and skills Be able to compare the mass, charge and location of the 3 subatomic particles. Know the difference between mass number and atomic number. Be able to calculate the atomic weight of an element when given information about the element’s isotopes. Be able to determine the number of subatomic particles in atom from incomplete information about the element. Be able to describe Bohr’s model of the atom. Be able to describe Thomson, Dalton and Rutherford’s contribution to the development of the atomic model. Know the 5 statements of Dalton’s atomic theory and be able to describe any shortcomings. Be able to explain how a line emission spectrum is created. Be able to write electronic configurations for elements. Be able to describe the 4 quantum numbers. Be able to identify electron configurations for elements in the excited state. Be able to write electron configurations for ions. Be able to give the values of the quantum numbers for a given orbital. Be able to list the types of light in the electromagnetic spectrum based on energy, frequency or wavelength.

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Subatomic particles Electron mass = 0amu charge = -1 location: in orbitals Proton mass = 1amu charge = +1 location: in nucleus Neutron mass = 1amu charge = 0 location: in nucleus Atomic number = protons in atom (and electrons in a neutral atom) Mass number = protons + neutrons 2 notations to know: C-12 (means the element Carbon with mass number 12) Or (where 6 is the atomic number and 12 is the mass number)

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Subatomic particles – sample questions Determine the number of protons, neutrons and electrons in: a. Nickel-58. b. Nickel-602+ c. d. Ca2+ Determine the numbers of each of the subatomic particles in: a. An element with atomic number 5 and mass number 13 b. An element with mass number 37, with 17 electrons 3. How many neutrons are present in an atom of tin that has the atomic number 50 and a mass number of 119?

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Isotopes and atomic weight Isotopes are atoms of an element that have the same number of protons but a different number of neutrons (and therefore different mass numbers) To calculate the atomic weight of an element: Atomic weight = (mass of isotope 1)(abundance of isotope 1) + (mass of isotope 2)(abundance of isotope 2)

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Isotopes and atomic weight- Sample questions Element Q consists of 3 different isotopes, A, B and C. Isotope A has an atomic mass of 40amu and accounts for 60% of naturally occurring Q. The atomic mass of isotope B is 44amu and accounts for 25% of Q. Finally, isotope C has an atomic mass of 41amu and a natural abundance of 15%. What is the atomic weight of element Q? The mass of a copper-63 atom is 62.94amu and that of a copper-65 atom is 65.93amu. Using this data and the abundance of these two isotopes, determine the average atomic mass of native copper. The abundance of copper-63 is 69.17%. The abundance of copper-65 is 30.83%. Which of the following could represent a pair of isotopes? a. b. c. d.

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Bohr’s model of the atom Bohr thought that in atoms electrons rotated around the nucleus in precise orbits. Electrons could move from low energy orbits (close to the nucleus) to high energy orbits (further away) by absorbing energy. When electrons moved back down to the low energy orbit they give off energy in the form of light. The many electrons in a substance moving from high energy orbits to low energy orbits, giving off light energy creates lines of color in what is called a line emission spectrum.

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP The Quantum mechanical model of the atom Electrons are found in 3D regions of space, called orbitals (not rings or orbits). Orbitals are the region of space where the electron is likely to be found 90% of the time. Orbitals in atoms have different shapes(s, p, d, and f), sizes and energies. Electrons are described with 4 quantum numbers: Principal quantum number (n), angular momentum quantum number(l), magnetic quantum number (ml)and the spin quantum number(ms) There are rules that specify what values the quantum numbers can have: n = 0, 1, 2, 3, 4… l = 0, 1, 2, 3…(n-1) ml = -l…0…1 ms = ±1/2

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP The Quantum mechanical model of the atom – sample questions Calculate the maximum number of electrons that can occupy the 4th principal energy level. Write the orbital diagram for Aluminum. Explain what law the following configuration violates. 1s22s32p63s1 The maximum number of electrons with quantum numbers n = 2 and l = 1 in one atom is ____. How many subshells are found in the 3rd principal quantum level? How many orbitals are there in the 5d subshell? The location of an electron is identified by the atomic orbital it is in. Which properties of an atomic orbital are specified by the first three quantum numbers? a. Length, width, and height d. Size, exact location and velocity b. Mass, speed and direction e. Color, frequency and wavelength c. Size, shape and orientation

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Electron configurations The order of the orbitals is: 1s 2s 2p 3s 3p 4s 3d 4p 5s Each s-sublevel can hold 2 electrons Each p-sublevel can hold 6 electrons Each d-sublevel can hold 10 electrons Electronic configurations can be written by filling in the electrons in the orbitals starting with the lowest energy.

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Electron configurations – Sample problems What is the lowest energy orbital in an atom? Write the electron configuration for Boron. Write the electron configuration for Ca2+ Write the electron configuration for copper. Write the electron configuration for Cl- 6. Which of the following electron configurations corresponds to an excited state? 1s22s23p1 1s22s22p6 1s22s22p43s1 [Ar] 4s23d54p1 Which of the following is the ground-state electron configuration of an oxide ion? a. 1s22s22p4 b. 1s22s22p5 c. 1s22s22p6 d. 1s22s22p63s1 e. 1s22s22p63s2

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP MORE PROBLEMS

Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Key terms Halogens Noble gases Alkali metals Alkaline earth metals Metals Nonmetals metalloids Period Group/family Valence electrons Modern periodic law Mendelev S block P block D block F block Octet rule Atomic radius Ionization energy Electronegativity First ionization energy Electron affinity Malleability Ductility Transition elements Ionic radius

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Key concepts and skills Know the periodic trends for: atomic radii, ionization energy, electronegativity, electron affinity, reactivity, boiling point, density. Know the modern periodic law. Know why elements in the same group have similar chemical properties. Be able to determine the number of valence electrons an element has based on its position in the periodic table. Know the location of metals, nonmetals and metalloids in the periodic table. Know basic properties/characteristics of groups. Know the location or the s,p , d and f blocks in the periodic table. Be able to determine an element’s valence electrons and ions formed from its position in the periodic table.

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Periodic trends Electronegativity: increases from left to right and down to up. Atomic radius: increases from right to left and up to down. Ionization energy: increases from left to right and down to up. Electron affinity: increases from left to right and from down to up.

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Periodic trends-sample questions In which of the following pairs is the first element expected to have a higher electronegativity than the second? a. O, P b. Cs, Rb c. I, Br d. Al, P e. Sb, As In which pair of elements is the larger atom listed first? a. K, Ca b. Na, K c. Cl, S d. Mg, Na e. O, N

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table Elements in periodic table are ordered by increasing atomic number. Elements in the same groups have the same number of valence e’s which explains why they have similar chemical properties. The blocks of the table are s, d, p (from left to right). S-block elements are Groups 1 and 2 D-block elements are in Groups 3-12 P-block elements are in Groups 13-18 To determine an element’s valence electrons: For Group 1 and 2 group number = # valence electrons For Group 13-18 group number -10 = # valence electrons

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table – sample questions A solid element has 2 valence electrons. That element must be: a. A halogen b. A noble gas c. A radioactive element d. An alkali metal e. An alkaline earth metal The differentiating electrons for transition elements are: a. D electrons b. S electrons c. P electrons d. F electrons e. Valence electrons 3. How many protons, neutrons and electrons are in an atom of Bromine? Chemical properties of elements are defined by the____________. a. Electrons b. Ionization energy c. Protons d. Neutrons e. electronegativity

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table – sample questions Which pair of elements is expected to have the most similar properties? a. Potassium and lithium b. Sulfur and phosphorus c. Silicon and carbon d. Strontium and barium e. Fluorine and iodine

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS

Lesson 1 Nuclear chemistry : Lesson 1 Nuclear chemistry SAT II PREP Key terms Nucleus nuclide Nucleon Atomic number Mass number Isotope Atomic mass unit Nuclear binding energy Mass defect Radioactivity Radioactive decay Fusion Fission Daughter isotope Parent isotope Alpha particle Alpha decay Beta particle Beta decay Gamma ray Gamma decay Positron emission Electron capture Half life Exponential decay Carbon dating Decay constant Transmutation Nuclear chain reaction

Lesson 1 Nuclear chemistry : Lesson 1 Nuclear chemistry SAT II PREP Key concepts and skills Be able to identify isotopes. Be able to solve half-life and radioactive decay problems. Be able to balance nuclear equations. Know the key characteristics of the subatomic particles: positron, beta particle, alpha particle, gamma ray, etc. Be able to classify nuclear reactions by looking at their equations. Be able to explain mass defect and binding energy. Be able to describe how the nucleus changes in different types of radioactive decay processes. Be able to distinguish between fission, fusion, radioactive decay and transmutation.

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Subatomic particles

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Types of nuclear reactions Beta decay Fission of uranium Electron capture Fusion reaction Positron emission Alpha decay C 14 6 N 14 7 + e 0 -1 Cr 51 24 V 51 23 + e 0 -1 + ? Cr 49 24 V 49 23 e 0 +1 + U 238 92 Th 234 90 He 4 2 + U 92 n 1 0 + Ba 87 35 + La 146 57 + 3 n 1 0 235 H 2 1 He 4 2 + H 3 1 + n 1 0

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Types of nuclear reactions- sample questions The radiation given off by iodine-131 in the form of beta particles is used to treat cancer of the thyroid gland. Write the nuclear equation to show what happens when an iodine-131 nucleus decays. The decay of uranium-238 results in the spontaneous ejection of an alpha particle. Write the nuclear equation that describes this process. When a radon-222 nucleus decays, an alpha particle is emitted. Write the nuclear equation to show what happens when a radon-222 nucleus decays. What is the other product that forms? A fusion reaction that takes place in the sun is the combination of two helium-3 nuclei to form 2 hydrogen atoms and one other atom. Write the balanced nuclear equation for this fusion reaction. Be sure to include both products that are formed.

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Balancing nuclear equations The total of the superscripts on the left side of the equation must equal the total of the superscripts on the right side of the equation. The total of the subscripts on the left side of the equation must equal the total of the subscripts on the right side of the equation. Summary of effect of different nuclear changes Emission of a beta particle: increases atomic number by one but does not change the mass number. Emission of a positron: decreases the atomic number by one but does not change the mass number Electron capture: decreases the atomic number by one but does not change the mass number Alpha decay: decreases atomic number by 2 and the mass number by four.

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Balancing nuclear equations – sample questions Write balanced equations for the following nuclear reactions: a. Uranium-233 undergoes alpha decay. b. Copper-66 undergoes beta decay. c. Beryllium-9 and an alpha particle combine to form carbon-13. The carbon-13 nucleus then emits a neutron. d. Uranium-238 absorbs a neutron. The product then undergoes successive beta emissions to become plutonium-239 2. Write in the missing particle in the following nuclear reactions. Mn 55 25 n 1 0 + He 4 2 + Np 239 93 Pu 239 94 + C 11 6 B 11 5 + Li 6 3 n 1 0 + He 4 2 + U 235 92 n 1 0 + Ba 139 56 + Fr 94 36 + 3

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Half-life and radiactive decay calculations Half life is the time required for one half of a radioactive sample to completely decay. Two equations to know: N/No = e-kt N is the amount of the radioactive sample at some later time, t. No is the original amount of the radioactive sample. k is the rate constant t is the time that the sample decays for t1/2 = 0.693/k k is the rate constant

Lesson 1 Nuclear Chemistry : Lesson 1 Nuclear Chemistry SAT II PREP

Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Half-life and radiactive decay calculations- Sample questions Part A Simple ½ life problems A radioactive substance has a half-life of 20 minutes. If we begin with a 500 g sample, how much of the original sample remains after two hours? How much of a 100.0g sample of Au-198 is left after 8.10 days if gold’s half-life is 2.70days? After a 50.0g sample of N-16 decays for 14.4 seconds 12.5g of the original sample remains. What is N-16’s half-life? Part B ½ life problems that require equations & calculation The half-life of Ag-104 is 16.3 min. What is the rate constant in units of reciprocal seconds (s-1)? Bromine-82 has a half-life of 35.7 hours. How many milligrams of Br-82 will remain if 2.30g of Br-82 decays for exactly one week? After 3.24 hrs 75% of a radioactive substance is left. What is the rate constant in units of reciprocal hours?

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Key terms Molecule Chemical bond Valence electrons Intermolecular forces Intramolecular forces Octet rule Ionic bonds Covalent bonds Polar covalent bonds Cations Anions Polyatomic ions Double bond Single bond Triple bond Bond length Bond energy Lewis structures Formal charge Resonance structures Partial charge Nonpolar covalent bonds Coordinate covalent bonds VSEPR Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral Dipole moment Hybridization sp hybridization sp2 hybridization sp3 hybridization Sigma bond Pi-bond W o r d s 2 k n o w

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Molecule Chemical bond Valence electrons Intermolecular forces Intramolecular forces Octet rule Ionic bonds Covalent bonds Polar covalent bonds Cations Anions Polyatomic ions Double bond Single bond Triple bond Bond length Bond energy Lewis structures Formal charge Resonance structures Partial charge Nonpolar covalent bonds Coordinate covalent bonds VSEPR Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral Dipole moment Hybridization sp hybridization sp2 hybridization sp3 hybridization Sigma bond Pi-bond Concept Map

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Key concepts and skills Be able to draw lewis structures (and resonance structures when necessary). Be able to explain why some covalent bonds are more or less polar than others. Be able to determine formal charges on atoms in a molecule. Know the octet rule. Be able to draw lewis dot diagrams for ions. Know the most likely ions formed by main group elements. Know what kinds of bonds (pi/sigma) make up single, double and triple bonds. Be able to predict whether a molecule will be polar or not. Be able to predict the shapes of molecules. Be able to explain the differences between nonpolar and polar covalent bonds. Know the relative bond energies and length for single, double and triple bonds. Know the naming system for ionic and molecular compounds (know names of common polyatomic ions). Be able to do these things.

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Bond Polarity

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Bond Polarity

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Polyatomic Ions PO43- CO32- PO33- NO3- SO42- HCO3- ClO4- ClO3- phosphate chlorate sulfate perchlorate carbonate nitrate phosphite hydrogen carbonate

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dots P O2- F- N S H Cl C

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures for molecules

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures for molecules O2 CO NH3 CO2 BCl3

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures & resonance CO32-

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP VSEPR theory predicts shapes of molecules

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP 4 sp3 hybrid orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP 3 sp2 hybrid orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals Bonding in Ethene C2H4

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals 2 sp hybrid orbital

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals Bonding in Ethyne C2H2

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals

Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Solutions to problems

Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Solutions to problems