Atomic Structure & Periodicity Name:
Study Guide
Date: Per:
Directions: Complete the questions below in preparation for the exam. I will not go over the study guide in class, but I am available after school for individual questions. The test format is 18 multiple choice, and7 short answer. Calculations will be included in both sections.
Learning Targets for Unit 3: Atomic Information & Periodicity
- Atomic Information
- State the location and charges of each subatomic particle within the atom
- Use the periodic table to determine the number of protons, neutrons, and electrons in an atom of an element
- Define atomic number as it relates to subatomic particles
- Define atomic mass as it relates to subatomic particles.
- Draw a Bohr Model of an atom, given its atomic notation
- Identify the number of valence electrons from a diagram or Bohr Model
- Isotopes and Relative Atomic Mass-
- Explain and illustrate the concept of isotopes
- Explain the concept of relative atomic mass
- Calculate the atomic mass of an element, given the mass and abundance of naturally occurring isotopes
- Use isotope notation to determine the number of protons, neutrons, and electrons for an isotope of an element.
- Write an isotope symbol when given information about the number of subatomic particles in an isotope of an element.
- Nuclear Reactions
- Describe half-life as the amount of time it takes for half of a radioactive sample to decay
- Perform basic half-life calculations
- Compare the energy outputs of fission and fusion reactions
- Energy Levels and Electron Configuration
- State the energy sublevels within an energy level
- State the maximum number of electrons that can occupy a given energy level and sublevel
- List the order of sublevels according to increasing energy
- Write the predicted electron configuration for the first 20 elements
- Identify the number of valence electrons from an electron configuration
- Electron Dot Diagrams – Draw electron dot diagrams for the first 20 elements.
- Ions
- Describe how distance effects the attraction between protons and neutrons
- Describe the formation of ions as either a gain or loss of electrons
- Describe the formation of ions in terms of oxidation and reduction
- Determine ion charge based on the number of valence electrons present in the neutral atom
- Predict the ion charge based on location on the periodic table
- Determine if an ion is a cation or anion
- Groups and Periods on the Periodic Table- Periodic Law
- Define group as it relates to the periodic table.
- Define period as it relates to the periodic table.
- Periodic Trends (number of valence electrons, atomic radius- include effective nuclear charge, electronegativity, ionization energy)
- Discuss the trends in valance electrons as you move from left to right and top to bottom on the periodic table.
- Discuss the trend in atomic radius as you move from left to right and top to bottom of the periodic table.
- Discuss the trends in electronegativity as you move from left to right and top to bottom of the periodic table.
- Discuss the trends in ionization energy as you move from left to right and top to bottom of the periodic table.
- Properties of Elements- 1A, 2A, 7A, 8A
- Discuss the properties of alkali metals.
- Discuss the properties of alkali earth metals.
- Discuss the properties of halogens.
- Discuss the properties of noble gasses.
Practice Questions
- Complete the following table.
Subatomic Particle / Charge? / Location in the atom? / How do you determine it from the periodic table?
Proton
Neutron
Electron
- Consider the following:
- What is the atomic number?
- What is the atomic mass?
- How many protons?
- How many neutrons?
- How many electrons?
- Consider the following: Silicon-30
- Write the atomic/isotope notation.
- Draw a Bohr model.
- How many valence electrons?
- Define isotope.
- Rubidium has two isotopes, Rubidium-86 with a mass of 86.03 (52%) and another isotope. If the average atomic mass of Rubidium is 85.47, what is the other isotope?
- Write and solve your own average atomic mass problem using Platinum
- How much of a 20.0g sample of a radioactive substance would remain after 6 half-lives?
- If 100g of a sample of radioactive substance is remaining after 7000 years, and the half-life of the substance is 125 years, how much of the substance was originally present?
- Write and solve your own half-life radioactive decay problem
- Define fission. How could you recognize if a fission reaction was illustrated?
- Define fusion. How could you recognize if a fusion reaction was illustrated?
- Draw the Lewis Dot Diagram for Calcium
- Write an electron configuration for a neutral atom of Arsenic
- Identify the energy levels by circling them.
- Identify the energy sublevels by underlining them.
- Put a box around the electrons.
- Highlight the valence electrons.
- If Arsenic forms an ion, will electrons be gained or lost?
- What charge will an ion of arsenic have?
- Write the isotope notation for the ion of arsenic?
- Is an ion of arsenic a cation or anion? Explain your reasoning.
- Describe how ions form.
- Define the following terms and discuss the trends on the periodic table in relation to each term. Be sure your description clearly identifies why each trend exists.
- Valence electrons
- Energy level
- Atomic radius
- Electronegativity
- Ionization energy
- Coulombic attraction
- Reactivity
- Define group and period as they relate to the periodic table. What do elements in the same group have in common? What do elements in the same period have in common?
- Consider the following element: Phosphorous (Zn).
- Write the atomic/isotope notation.
- Write the ground state electron configuration.
- Draw the orbital diagram for the neutral atom (the boxes with arrows)
- On the periodic table below, label the following:
- Number the groups (1A-8A)
- Number the periods
- Representative elements
- Transition metals
- Inner transition metals
- Metalloids
- Alkali metals
- Alkali earth metals
- Halogens
- Nobel gasses