Midterm Review Sheet (TEST Grade) PDF

Midterm Review Sheet: Complete question answers on a separate sheet of paper for a TEST Grade Completed by Thursday **Schedule for Homework through the week** Friday Night Due Monday:Lab Safety and Chapter 1 Monday Night Due Tuesday: Chapter 3 and Chapter 2 Tue...

Midterm Review Sheet: Complete question answers on a separate sheet of paper for a TEST Grade Completed by Thursday **Schedule for Homework through the week** Friday Night Due Monday:Lab Safety and Chapter 1 Monday Night Due Tuesday: Chapter 3 and Chapter 2 Tuesday Night Due Wednesday: Chapter 4 and Chapter 5 Wednesday Night Due Thursday: Chapter 6 and Chapter 7 Lab Safety 1. Why is it important to wear safety goggles in the chemistry laboratory? 2. Why should you avoid eating, drinking, or chewing gum in the laboratory? 3. What should you do if a chemical spills? 4. What should you do if glassware breaks in the lab? 5. Why should unused chemicals not be returned to the reagent bottle? 6. How should you properly dilute an acid? 7. What are the dangers of leaving a lighted burner unattended? 8. Why is it important to stay clean and organized in the lab? 9. Why must loose hair and long jewelry be tied back? 10. Write a scenario where a lab safety rule is violated and suggest the correct actions to take. Chapter 1: Introduction to Chemistry 1. What is the definition of chemistry? 2. What are the five traditional areas of study in chemistry? 3. What is the difference between pure chemistry and applied chemistry? 4. What are three main reasons to study chemistry? 5. What is the difference between the macroscopic and microscopic worlds? 6. What are three main areas of research affected by chemistry? 7. Who was Antoine-Laurent Lavoisier, and what were his contributions to chemistry? 8. What are the steps of the scientific method? 9. What is the difference between an independent and dependent variable? 10. Define collaboration and communication. Why are they important in science? Chapter 3: Measurement, Unit Conversion, Dimensional Analysis, Significant Figures  1. What is the difference between accuracy and precision? 2. What is the difference between qualitative and quantitative observations? 3. How do you round measurements correctly based on increments? 4. What are the SI units for mass, length, temperature, time, and the amount of a substance? 5. What are the three units of temperature? 6. List the SI prefixes from Mega (M) to Micro (µ) and their exponential factors. *** You will need to know how to convert from one unit to another (MKHDDCMM) 7. How do you calculate area, volume, and density? 8. How many Sig Figs are in the following numbers? - 500 - 457 - 000.04506 - 0.00487 - 500. - 202 9. What is the rule for significant figures in multiplication/division? What about addition/subtraction? Solve: 4.5 x 600 Solve: 589.4 - 600.99 10. The football team needs 550 cm for a 1st down. How many yards is this? Given: 1 in = 2.54 cm 1 yard = 36 in **Know how to use dimensional analysis to solve a problem*** Chapter 2: Matter 1. What is matter? 2. What are compounds, elements, and atoms? 3. What are the four states of matter, and how are they identified in terms of volume and shape? 4. What is the difference between a physical change/property and a chemical change/property? 5. What are reactants and products? 6. What are the cues for a chemical reaction? 7. What is the difference between extensive and intensive properties? 8. Define mixture and describe the two types of mixtures. 9. What are the two ways to separate mixtures, and which type is each associated with? 10. What is a pure substance? What are the characteristics of pure substances?  11. How do you break down a compound? 12. What does the law of conservation of mass state? Chapter 4: The Atom 1. Who was Democritus, and what was his contribution to atomic theory? 2. What did Rutherford discover? 3. What are the three subatomic particles, their charges, and symbols? 4. How do you determine the mass number of an atom? 5. What is hyphen notation? Provide an example. 6. What is nuclear symbol notation? Provide an example. 7. What are ions and isotopes? 8. An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element. ****Know how to calculate the average atomic mass of an element Chapter 5: Atomic Models and Electron Behavior 1. What’s the order of Dalton, Thomson, Rutherford, Bohr, and Schrodinger’s atomic models? 2. What was the new proposal of Bohr’s atomic model? 3. What are energy levels, and what is a quantum of energy? 4. What does the quantum mechanical model represent? Where is the electron density highest? 5. What is an atomic orbital, and what are the shapes of s, p, d, and f energy sublevels? 6. Write an electron configuration for: Li C Mg N 7. Define amplitude, wavelength, frequency, and their units of measurement. ** know how to identify these on a diagram 8. What is the relationship between wavelength and frequency? 9. What is the speed of light, and how do you calculate frequency or wavelength? 10. If given a wave with a wavelength of 4.0 x 10^-7 (m) what is the frequency of the wave?  11. What is an atomic emission spectrum? What causes it? Chapter 6: The Periodic Table 1. Who were Dmitri Mendeleev and Henry Moseley? What did they contribute to chemistry? 2. What does the periodic law state? 3. How are elements arranged in the periodic table? 4. What are the properties of metals, nonmetals, and metalloids? 5. What happens to atomic radius, ionization energy, and electronegativity as you move down a group and across a period? 6. What are cations and anions? How does the size of an atom change when electrons are added or removed? 7. What is electron affinity, and how does it change across a period or down a group? 8. What happens to melting points, boiling points, and density as you move down a group or across a period? ***Be able to identify key groups: Alkali Metals, Alkaline Earth Metals, Halogens, Noble Gases, etc. Chapter 7: ionic and Metallic Bonding 1. What are valence electrons, and where are they found in an atom? 2. Explain the Octet Rule and its importance in forming compounds. 3. What do atoms of metals typically do to achieve a stable electron configuration? 4. What do atoms of nonmetals typically do to complete the Octet Rule? 5. Define cations and anions and explain how each is formed. 6. What is an ionic bond, and how does it hold ionic compounds together? 7. Why are ionic compounds electrically neutral? 8. Describe what happens to the valence electrons of a metal in the "sea of electrons" model. 9. List three properties of ionic compounds. 10. Why are metals good conductors of electricity? 11. How do the properties of alloys compare to the properties of the pure metals that compose them? 12. Write the ionic charge for elements in: a) Group 1A b) Group 2A c) Group 6A 13. Give an example of a transition metal ion and explain why its charge is shown with a Roman numeral. 14. What is a formula unit, and how does it relate to ionic compounds? 15. Why do ionic compounds have high melting points? 16. Explain how alloys are created and why they are useful.