Exam 1 Content List PDF

Overall Tips: 1.) Review the video assignments and your notes. Make sure to study the questions you saw in lab that I have put into the weekly assignments- a few will make the exam cut. 2.) Make a study sheet with important terms to memorize and important concepts. 3.) Review in class activities...

Overall Tips: 1.) Review the video assignments and your notes. Make sure to study the questions you saw in lab that I have put into the weekly assignments- a few will make the exam cut. 2.) Make a study sheet with important terms to memorize and important concepts. 3.) Review in class activities (these are more practice from the video assignment) 4.) Do the extra practice problems. They are optional but are good practice. The extra problems can be found in each week in the “modules” by week (Example: Week 1 has a worksheet you can print out) and in week 2 there is a combination of a worksheet and two “Formatives” where you do your video assignments” there are some in week 2 and 3. 5.) If you have done all of this- you are in great shape! Learning Objectives Guide for Atomic Structure, Matter, and Units This guide provides the key content that you need to understand based on the learning objectives related to atomic structure, matter, and measurement units. 1. Units and Their Importance (week 3) Understand why units are important: understand that units allow scientists to measure and express quantities consistently. Units provide clarity, enable comparison, and facilitate communication of scientific findings. Recognize different systems of units: o Metric: Meter (m), Gram (g), Liter (L) o English: Inches, Pounds, Gallon Expressing measurements: You need to be able to convert between different metric units of length, volume, and mass. For example, converting from grams to kilograms, and liters to milliliters. Memorize prefixes kilo, centi, milli 2. Matter and States of Matter Definition of matter: You must know that matter is anything that has mass and occupies space. Know “States” of matter: o Solid: Fixed shape and volume. o Liquid: Fixed volume but no fixed shape, takes the shape of its container. o Gas: No fixed shape or volume, expands to fill its container. 3. Atomic Structure and Elements Know key atomic concepts and terms Protons: Positive charge (+1), mass = 1 amu. Electrons: Negative charge (-1), mass = negligible (1/1836 of proton). Neutrons: Neutral charge (0), mass = 1 amu. Atomic mass: the sum of the proton and neutrons Charge: protons - electrons Isotope: Atoms of the same element with different numbers of neutrons, leading to different atomic masses. Element: A substance made of only one type of atom, defined by the number of protons present. Know and be able to use formulas for calculating charge and atomic mass Be able to use atom notation and determine missing information (charge, neutrons, protons, electrons) Know definitions: o Ion: An atom that has gained or lost electrons to form a charge. o Anion: Negatively charged ion o Cation: Positively charged ion Elements 1-18 Be able to recall the names and symbols of the first 18 elements on the periodic table (e.g., H = Hydrogen, He = Helium, etc.). Atomic 3-D Structure and Electrostatics Electrostatic Attraction and Repulsion: o Opposite charges attract (protons and electrons). o Electrons repel electrons. Nucleus: Center of the atom, containing protons and neutrons, most of the atom’s mass. Orbitals: Regions in space around the nucleus where electrons are most likely to be found. o s orbital: Spherical shape, 1 orbital o p orbital: Dumbbell shape, 3 orbitals o d orbital: Clover (don't need to know name clover) shape, 5 orbitals o f orbital: More complex shapes, 7 orbitals 5. Electron Configuration and Energy Electron Configuration: The arrangement of electrons in an atom’s orbitals. o Electrons fill the lowest-energy orbitals first. ▪ Which is lowest energy and why? ▪ Each orbital can hold a maximum of two electrons with opposite spins. (why is out of scope of the class) ▪ Electrons fill energy orbitals of the same energy (example p orbitals) singly before pairing up to minimize repulsion. Energy and Orbital Diagrams: o Orbitals: Electrons fill orbitals from lower to higher energy levels. o Energy Diagram: The relative energies of orbitals and how electrons fill them in order. Electron Configuration of Elements 1-20: Students should be able to write the full electron configuration for elements 1-20, such as: o H (Hydrogen): 1s¹ o He (Helium): 1s² o Li (Lithium): 1s² 2s¹ o and so on up to Ca (Calcium). 6. Practice Problems and Activities Practice writing electron configurations for elements. Practice drawing orbital energy diagrams to show electron arrangements. Use energy level diagrams to illustrate how electrons fill orbitals. 7. Key Concepts to Review: Units: Convert between metric and English units, and apply units to measure length, mass, volume, and density. Atomic Structure: Understand the components of an atom and how they determine an element’s properties. Electron Configuration: Be able to write configurations for elements and explain how energy levels affect stability. Atomic Structure and Energy: Understand how energy influences electron behavior and orbital filling. Key Concepts: Forces and Energy Force: Interaction between objects that causes either attraction (pull) or repulsion (push). Energy: The ability to do work or cause change. Charge Interactions: o Opposite charges (protons and electrons): Attract each other, lowering energy. o Electrons: Repel each other, increasing energy. o Distance’s Impact: The closer opposite charges are, the stronger the attraction and lower the energy. For like charges, the closer they are, the greater the repulsion and higher the energy. Energy States and Stability Systems tend to move toward more stable, lower energy states.  Skydiving Example: Skydivers are higher in energy at the top (high in the sky) and lose energy as they fall, reaching a more stable, lower energy state when they hit the ground. Be able to compare interactions between 2 magnets and protons/electrons Example: o Repelling Magnets: Higher energy state (unstable). o Attracting Magnets: Move to a more stable, lower energy state (more stable) 5. Charge Interactions and Energy Opposite Charges: Attraction lowers energy. Electron/electron repulsion increases energy. Charge Distance: o Opposite charges closer = stronger attraction, lower energy. o Electrons closer = stronger repulsion, higher energy. Summary of Key Energy Principles Forces cause changes in energy and stability. Objects and systems tend to move towards lower energy states for greater stability. Charge interactions (attractive or repulsive) directly affect the energy level and stability of a system. Periodic Table and its organization Use the periodic table to identify metals, metalloids, and nonmetals. Use the periodic table to identify alkali metals, alkaline earth metals, transition metals, halogens, noble gases Know the terms group and period in relation to the periodic table. Make connections between the elements and everyday living Define an element Know elements 18-36 names and their corresponding symbols (for exam 2) Describe what a diatomic molecule is and identify the seven elements found in nature as diatomic molecules.