Name Chemistry Review



Download 264.85 Kb.
Page1/3
Date23.04.2018
Size264.85 Kb.
  1   2   3
Name ___________________

Chemistry Review

Chm.1.1 Matter:Properties and Change 

Chm. 1.1.1

Analyze the structure of atoms, isotopes, and ions.

Chm. 1.1.2

Analyze an atom in terms of the location of electrons.

Chm. 1.1.3

Explain the emission of electromagnetic radiation in spectral form in terms of the Bohr model

Chm. 1.1.4

Explain the process of radioactive decay by the use of nuclear equations and half-life.



Big Ideas

Essential Questions

         Know the location and charge of protons, neutrons, electrons

         Determine an element’s number of protons, electrons, and neutrons based off the given isotopic symbols

         Differentiate average atomic mass of an element from the actual isotopic mass and mass number of specific isotopes

         Analyze electrons in terms of

•         Bohr model

•         Excited stated vs. ground state

•         Emission spectrum (Reference Table)

•         electron configurations

•         wave/particle duality 

         Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency. 

         Write and balance nuclear equations

         Describe nuclear decay

         Compare fission and fusion

         Understand half-life problems



  • How can atomic models be used to describe and explain the structure of atoms?

  • In what ways has the theory of the atom changed over time due to technological developments?

  • What is the law of conservation of mass?

  • What is the law of definite proportions/multiple proportions?

  • What were the 5 points to Dalton’s atomic theory?

  • How was the use of cathode rays responsible for the discovery of the electron?

  • How did Rutherford’s experiment lead to the discovery of the atomic nucleus?

  • What are the properties (charge, mass, position) of protons, neutrons, and electrons?

  • What is an isotope?

  • What is the atomic number of an atom equal to?

  • What is the mass number of an atom equal to?

  • Why is the mass number in the periodic table a decimal?

  • How is the wave-particle duality explanation used to explain light and electrons?

  • What is the relationship between the speed, frequency, and wavelength of electromagnetic radiation?

  • What is the significance of the photoelectric effect in describing the behavior of the electron and light?

  • How did the Heisenberg Uncertainty Principle and the Schrödinger Wave equation lead to atomic orbitals?

  • What are the downfalls of the Bohr model of the atom?

  • What are the differences between the Bohr model and the Quantum model of the atom?

  • What is the significance of each of the four quantum numbers?

  • How are the quantum numbers used to describe the position of an electron in an atom?

  • How many electrons fill each energy level and each orbital?

  • What is the significance of the Aufbau principle, the Pauli Exclusion Principle, and Hund’s rule when discussing electron configuration within the atom?

  • Given an element, how do I determine its electron configuration, orbital notation, and electron dot notation?

  • How are nuclear reactions used to describe nuclear decay

  • How do nuclear fission and nuclear fusion reactions differ?



Atom

Atomic mass

Atomic mass unit

Atomic number

Electron

Ion


Isotope

Mass number

Neutron

Nucleus


Proton

Bohr Model

Electron

Electron cloud

Electron configurations


Emission Spectra

Energy level

Orbital

Sublevel


Electromagnetic radiation

Emission spectra

Energy

Energy level



Frequency

Nucleus


Orbital

Photon


Quanta

Sublevel


Wavelength

Fission


Fusion

Half life

Nuclear Decay

Radioactive decay





Student Performance Goals

Learning Targets

Criteria for Success

I will…


I can…


  • Be able to look at the periodic table and determine the number of protons, electrons and neutrons and elements has

  • Determine number of protons, electrons, and neutrons when given an isotopic symbol

  • Tell the difference between average atomic mass and mass number

  • Draw an elements Bohr Model

  • Be able to determine electron configurations for elements

  • Manipulate and solve C = 

  • Use and understand the electromagnetic spectrum

  • Be able to write and balance nuclear equations use alpha and beta particles

  • Explain nuclear fission and fusion

  • Successfully work through half-life problems




  • Correctly calculate the number of protons, neutrons and electrons for all elements

  • Describe the difference between average atomic mass and mass number

  • Correctly draw Bohr Models for all elements making sure to include the nucleus and energy levels in which to place the electrons

  • Write the correct electron configurations for all elements making sure to include the s, p, d, f in the appropriate order

  • Use the numbers given to me in word problems to solve the wavelength formula and then use the numbers locate the appropriate area on the electromagnetic spectrum

  • Correctly write and balance nuclear equations using the knowledge that undergoing alpha decay produces an alpha particle and undergoing beta decay produces a beta particle.

  • Correctly describe nuclear fission is the splitting of one nucleus into two or more smaller nuclei and nuclear fusion is the joining of two or more nuclei into one nucleus

  • Use given information to solve radioactive half-life problems

Chm. 1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties

Chm. 1.2.1

Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds

Chm. 1.2.2

Infer the type of bond and chemical formula formed between atoms

Chm. 1.2.3

Compare inter- and intra- particle forces

Chm. 1.2.4

Interpret the name and formula of compounds using IUPAC convention

Chm. 1.2.5

Compare the properties of ionic, covalent, metallic, and network compounds



Big Ideas

Essential Questions

         Predict bond type based off location of elements on the periodic table

         Determine positive and negative charge of element based off location of element on periodic table

         Predict chemical formulas

         Write and name binary chemical formulas/compounds

         Write and name compounds using Polyatomic Ions

         Know names and formulas for common acids

         Describe intermolecular forces for molecular compounds

         Explain the strengths and characteristics of intermolecular forces, ionic, covalent, and metallic bonds

         Explain the strengths of hydrogen bonds, dipole-dipole forces, and London Dispersion forces

         Apply and explain VSEPR with respect to molecular geometry

         Compare/Contrast polarity vs. nonpolarity

         Describe macromolecules and network solids



  • How does the distribution of electrons in atoms affect the formation of a compound?

  • What factors determine the types of chemical bonds that form between particles?

  • How do elements form ionic bonds?

  • How do elements form covalent bonds?

  • Are all electrons shared equally?

  • How are the properties of metals explained through metallic bonding?

  • How are the names of compounds determined (inorganic and acids)?

  • How are the formulas for compounds written?

  • How can I translate between a compound's name and its formula?

  • How can the charges of ions be used to determine balanced formulas involving polyatomic ions?

  • How can we predict the shape, structure and properties of molecules?

  • What is the difference between ionic, covalent, and metallic bonding?

  • How do intramolecular and intermolecular forces affect properties of a compound?



Anion

Cation


Covalent Bond

Electron Dot Structure/Diagram (Lewis Dot Structure/Diagram)

Ionic Bond

Metallic Bond

Valence Electron


Chemical Formula

Ionic Bond

Lewis Structure

Periodic Table

Covalent Bond

Diatomic Molecule

Dipole-Dipole Forces

Hydrogen Bond

Intermolecular Forces

Intramolecular Forces

Ionic Bond

London Dispersion Forces

Metallic Bond

Polar Bond



Binary Compound

Metal


Molecule

Nomenclature

Nonmetal

Polyatomic Ion


Covalent Bond

Ionic Bond

Ionic Compound

London Dispersion Forces

Metallic Bond

Molecular Compound

van der Waals Forces

VSEPR




Learning Targets

Criteria for Success

I will…


I can…


  • Be able to distinguish the difference between bond type and characteristics

  • Be able to predict bond type when given elements

  • Be able to draw ionic bonding diagrams

  • Write chemical formulas

  • Name chemical compounds

  • Write chemical formulas and name compounds using polyatomic ions

  • Determine VSEPR Shape

  • Determine Polarity/NonPolarity

  • Be able to explain intermolecular forces

  • Be able to distinguish between a network solid and a macromolecule.

  • Explain the characteristics of covalent, ionic, and metallic bonds

  • Examine elements given and based off their location on the periodic table determine if they will form a binary covalent, ionic, or metallic bond

  • Use Lewis structures to draw ionic bonding diagrams

  • Use ionic bonding diagrams to determine cationic and anionic charges of the elements.

  • Determine charges of elements and use the cross down method to write chemical formulas

  • Use the correct IUPAC systems (include Stock and Greek Systems) to correctly name compounds

  • Name and write compounds containing polyatomic ions

  • Draw the correct molecular geometry shape for covalent compounds and determine the correct VSEPR shape

  • Explain the concept behind the VSEPR theory

  • Draw correct VSEPR shapes for covalent compounds and determine if they are polar or nonpolar

  • Explain the difference between inter- and intra- molecular forces

  • Explain the differences between all the intermolecular forces

  • Distinguish the difference between a macromolecule and a network solid

Chm. 1.3 Understand the physical and chemical properties of atoms based on their position on the Periodic Table

Chm. 1.3.1

Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition)

Chm. 1.3.2

Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an elements based on its position on the Periodic Table

Chm. 1.3.3

Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.



Big Ideas

Essential Questions

         Identify groups as vertical columns on the periodic table

         Know that main group elements have similar properties, have the same number of valence electrons, and  same oxidation numbers

         Identify periods as horizontal rows on the periodic table

         Know the location of metals, nonmetals, and metalloids on the periodic table

         Use electron configuration to justify metallic character

         Using the periodic table, define and know the period and group trends of:

•         Atomic radius

•         Electron affinity

•         Ionization energy

•         Electronegativity

         Arrange elements in order of increasing or decreasing atomic radius/electron affinity/ionization energy/electronegativity and explain reasoning behind the trend.





  • How does the placement of an element in the Periodic Table relate to its chemical and physical properties?

  • How does knowing trends on the Periodic Table help scientists predict properties of the representative elements?

  • What happens to the atomic radius as the atomic number increases across a period? Down a group?

  • What happens to the energy needed to remove an electron as the atomic number increases across a period? Down a group?

  • Why does atomic radius change as it does?

  • Why does the energy required to remove an electron change as it does?



Alkali Metal

Alkali Earth Metal

Group (Family)

Halogen


Meta

Metalloid

Noble Gas

Nonmetal


Oxidation Number

Period, Reactivity

Transition Element

Valence Electron



Anion Radius

Atomic Radius

Cation Radius

Electron Affinity

Electron Configuration

Electronegativity

Ionic Radius

Ionization Energy

Metallic Character

Octet


Oxidation Number

Valence Electron



Electronegativity

Ionization Energy

Reactivity




Learning Targets

Criteria for Success

I will…


I can…


  • Describe the arrangement of the modern Periodic Table in terms of identifying families

  • Describe elements in terms of number of metallic character, number of valence electrons, and number of oxidation numbers

  • State the general trend for and arrange elements according to

    • Atomic and ionic radius

    • Ionization energy

    • Electronegativity

    • Metallic character

    • Electron affinity

  • Be able to determine if elements will gain or lose electrons based off position on Periodic Table

  • Be able to arrange a group of 3 or 4 elements in increasing or decreasing order according to desired trend (atomic radius, ionization energy, ionic radius, electronegativity, electron affinity)

  • Be able to tell if elements are in the same family and have the same number of energy levels based off given properties

Chm.2.1 Energy: Conservation and Transfer

Chm. 2.1  Understand the relationship among pressure, temperature, volume, and phase



Chm. 2.1.1

Explain the energetic nature of phase changes

Chm. 2.1.2

Explain heating and cooling curves (heat of fusion, heat of vaporization, melting point, and boiling point)

Chm. 2.1.3

Interpret the data presented in phase diagrams

Chm. 2.1.4

Infer simple calorimetric calculations based on the concepts of heat lost equals heat gained and specific heat

Chm. 2.1.5

Explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitative and quantitative



Big Ideas

Essential Questions

         All chemical and physical changes involve energy transfer

         The amount of heat transferred in a chemical/physical change can be predicted (calculated) using a balanced chemical equation. It can also be measured quantitatively through experimental means and graphically represented

         Explain why gases are less soluble in warm water than cold water

         Investigate the difference in the boiling or freezing point of pure water and a salt solution

         Measure, plot, and interpret the graph of a phase diagram of a substance under various conditions

         Examine and interpret heating and cooling curves for various closed systems.

         Contrast heat and temperature, including temperature as a measure of average kinetic energy

         Know that energy is neither created nor destroyed

         Explain physical equilibrium

         Explain and understand the relationship between pressure, temperature, volume, and amount of gas



         Complete calculations of:



  • How is energy transferred in chemical systems?

  • How does the potential energy and kinetic energy of molecules change during thermodynamic processes?

  • How do heat, temperature and internal energy differ?

  • Why is absolute zero so named?

  • Why can all reactions be classfiied as exothermic and endothermic?

  • How much energy is required to change a substance?

  • How is energy converted between kinetic energy and potential energy in a chemical reaction?

  • How does the motion of particles affect the temperature and phase of a substance?

  • How does pressure affect particle motion and phase change?

  • What is the relationship between molecular motion and thermal energy?

  • What is the nature of energy transfer?

  • How do you calculate heat capacity?

         How do gases behave?

         How do changes in pressure, volume, and temperature affect a gas?



  • What impact does the world of gases have on your life?

  • What are the key parameters that define a gas?

  • How are pressure and volume related to each other?

  • How are volume and temperature related to each other?

  • How are temperature and pressure related to each other?

  • How does Kinetic Molecular Theory describe the behavior of gases?

  • What is pressure?

  • How does a gas exert pressure?

  • How do we measure pressure?



Celsius

Equilibrium

Joule

Kelvin


Kinetic Energy

Phase


Phase Change

Physical Equilibrium

Potential Energy

Vapor Pressure



Boiling Point

Cooling Curve

Endothermic

Exothermic

Heat of Fusion

Heat of Vaporization

Heating Curve

Melting Point

Specific Heat


Boiling Point

Melting Point

Phase Diagrams

Sublimation


Calorimetry

Closed System

Phase Change

Specific Heat



Avogradro’s Law

Combined Gas Law

Dalton’s Law

Ideal Gas Law

Kinetic Molecular Theory

Pressure

Solubility

Temperature



Volume


Download 264.85 Kb.

Share with your friends:
  1   2   3




The database is protected by copyright ©ininet.org 2020
send message

    Main page