Chemistry Midterm Study Guide 2024 PDF

Name:_________________________________________ Date:_____________________ Period: _________ 2024 Chemistry Midterm Study Guide Complete the following Midterm Review prior to the Midterm Exam. MATERIALS: Make sure to bring a PENCIL and a CALC...

Name:_________________________________________ Date:_____________________ Period: _________ 2024 Chemistry Midterm Study Guide Complete the following Midterm Review prior to the Midterm Exam. MATERIALS: Make sure to bring a PENCIL and a CALCULATOR to your midterm exam. YOUR REFERENCE SHEET WILL INCLUDE: 1) Periodic Table 2) SI Unit Prefixes 3) Electromagnetic Spectrum STUDY SKILLS: In addition to using this study guide, a good study technique is to use old tests and quizzes to help prepare for larger exams. Use the tests and quizzes we have taken so far this year to review the types of questions that may be asked of you on the midterm. Unit 1: Introduction to Chemistry Command Terms; Lab Safety; Scientific Method; SI Units; Lab Equipment & Measurement; Data Tables & Graphs; Accuracy, Precision & Error; Density COMMAND TERMS Command terms will be used throughout the exam. Make sure you know and understand the task being asked of you for each command term. 1 LAB SAFETY D _____ 1. If a large fire starts in the lab, cover the fire with: a. water b. baking soda c. trash can Od. fire blanket _____ C 2. Know the location of and how to use ____ in the classroom. a. chemicals b. acids O c. safety equipment d. beakers B _____ 3. Never ____ in the lab unless told to do so. a. wash your hands O b. eat or drink c. read instructions C _____ 4. Always use ____ to handle hot test tubes. a. scissors b. beakers O c. tongs d. flasks B _____ 5. If a chemical splashes in your eyes, the best response is to: a. rinse in the sink for 15 mins O b. rinse in the eyewash for 15 mins c. rinse in the safety shower for 15 mins d. no rinsing is required 6. What is the first action you should take if an accident occurs in the lab? Notify the teacher 7. State safety procedures to follow before, during, and after a lab. Before During After tiebacklonghair neverleaveexperiment unattended replace alllids putongoggles and apron notifyteacherof anyspills or _properlydispose ofwaste accidents read procedure carefullyandask useequipment asinstructed followall clean only upprocedures clarifying questions return goggles andapron be awareof surroundings readsafetyinfo only conduct experiment inthe wash hands procedure 2 SCIENTIFIC METHOD 1. Match the elements of experimental design with each of the statements below for this experiment. A student designs the following experiment: She fills five cups with water, each at a different temperature: 75°C, 60°C, 45°C, 30°C, and 15°C. The cups are identical, and all have the same amount of water in them. The only difference between the cups is the temperature of the water they hold. All five cups are put into a freezer at exactly the same time. The freezer is then opened at one-minute intervals, and the time needed to form the first visible ice crystal is measured. a) Question i b) c) Hypothesis Experiment d) Conclusion _____ If the temperature of water is closer to 0oC, then it will take less time to observe the first ice crystals. B _____ The time to see the first visible ice crystal is measured for each different temperature sample. C D _____ Water at higher temperatures will take longer to completely freeze. A _____ What freezes faster, hot water or cold water? 2. Fill in the steps of the scientific method based on the scenario below: Marcie is trying a new cookie recipe. She wants to see if the amount of baking powder she uses will make the cookies rise more. She makes three batches of cookies and changes the amount of baking powder for each batch. a. Observation:Sometimes she willbakethick cookies and other timesshe will bakethin cookies b. Question:Does theamount ofbaking powder sheusesmake the cookies rise c. Research:what is in baking powder Howdoes it affect the cookies while baking What in it that makes the cookies rise d. Hypothesis:The morethe baking powderthehigherthe cookies willrisebecause of airbubbles e. Experiment:Make 3 batches of cookies w thesamerecipe except for the amount bakingpowder Itsp 2 of tsp 3tsp i. Qualitative observation: change intexture creation ofairbubbles ii. Quantitative observations: heightthecookiesrised to f. Analysis: create a graph ÉIÉÉ g. Conclusion: Addmore bakingpowder to increaseheight of cookies 3 SI UNITS 1. State the SI units for the following quantities. a. Time: b. Length: Sm c. Mass: kg d. Temperature: e. Volume: f. Density:51mL g. Pressure: org cm KPa 2. For the following units, state the SI prefix that is being applied and the numerical value that the prefix represents. The first is completed for you as an example. Quantity Unit Prefix Numerical Value Mass µg micro 0.000001 Pressure kPa 1000 Volume mL m 001 Length cm centi 01 LAB EQUIPMENT & MEASUREMENT 1. Draw (or add a picture) and describe the function of each of the following pieces of lab equipment. a. Bunsen burner uses air gas to createflame toheat samples b. IIe Graduated cylinder used to measure approx liquid volumes c. if Erlenmeyer Flask used to holdliquids swirlsamples notmeasurevolume d. Beakers used tohold liquids not measure volume e. If Electronic Balance usedto measure approx mass of sample f. Eff Filter Paper used to catch solid particles lets liquid fitration particles pass through 4 2. Describe the best way to measure a liquid volume using a graduated cylinder. keep on evensurface crouch to eyelevel measure from bottomofmeniscus 3. Describe the best way to measure the mass of a powder on an electronic balance. on balance press ZERO addsample Place weighboat to weigh 4. When working with the Bunsen burner, which flame is the safety flame, blue or yellow? Explain. yellow lesshot easyto see The simplest way to determine how many digits to record in your measurement is to look at the smallest marking on your instrument. Each measurement needs to include every digit shown on the instrument, plus one extra estimated digit. For example, if an object measures in between the 25.1 and 25.3 cm marks, we would need to 25.12 estimate one extra digit, such as 25.14 cm. If another object on the same ruler measured exactly to the 25.1 cm mark, we still need to record one extra digit, so 25.10 cm. 6. Give the correct measurement to the correct number of digits. Remember that you must estimate the last digit in the measurement and include units in your answer. a) cm 2 93 cm _________________ b) 44.3 mL _________________ c) 38.2 mL ___________________ d) 30.1 C _________________ 5  DATA TABLES & GRAPHS 1. Plot the data on the graphing grids provided. Remember title, axis labels (with units!), and scale. a. Tip: To help you find your scale, make sure you divide the highest number you need to go up to by the number of gridlines available. 2. Draw the best-fit line with a straightedge. 3. Use your graph to determine the % of sugar of the unknown, and write this value in the table below. Percent of Sugar (%) Density of Solution (g/mL) 0 1.00 10 1.02 20 1.05 30 1.07 40 1.09 50 1.12 4 0107 60 1.14 Unknown: ____________ 1.06 27 015 CONCENTRATION of SUGAR SOLUTIONS 1.18 1.12 É or no Et 1.03 100 0 10 20 40 90 70 4. of PEAR Calculate the slope of your best fit line. Show your work and use correct units. 60 4 0 5 0.03411 6 ACCURACY, PRECISION, & ERROR 1. Compare and contrast accuracy and precision. Accuracy closeness ofmeasurement totruemeasurement giveinfo if h m Precision closenessof multiple measurements 2. Two students did three trials each of calculating the density of quartz glass. The students’ results are recorded below. The true value for the density of quartz is 2.20 g/cm3. Trial 1 (g/cm3) Trial 2 (g/cm3) Trial 3 (g/cm3) Average (g/cm3) Daisy 2.63 1.98 2.35 Flapjack 2.15 2.26 2.21 a) Which student had the highest degree of precision? ______________________ FLAPJACK b) Calculate the % errors for both students. (𝑒𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙 𝑣𝑎𝑙𝑢𝑒−𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒) % 𝑒𝑟𝑟𝑜𝑟 = 𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒 𝑥100 100 949 11000.45 FLAPJACK c) Based on your calculations above, Which student was the most accurate? ____________________ 3. State examples of random error that occurred during the Density Lab. of fluevation electronicbalance of Wateraccidentallyspillingout graduated cylinder 4. State examples of systematic error that may have occurred during the Density Lab. Not zeroing thebalance Notstartingat 0cmmark on ruler DENSITY 1. Jacob found a piece of sea glass at the beach and wanted to determine its density. He measured its mass, and used the water displacement method to find its volume. His data is summarized in the table below: Mass of Sea Glass Volume of Water Volume of Water + Volume of Sea Density of Sea (g) (mL) Sea Glass (mL) Glass (mL) Glass (mL)glint 5.81 10.0 11.8 18 3.23 a. Calculate the volume of the sea glass. Show your work and put your answer in the table. 11.8 10.0 1.86 b. Calculate the density of the sea glass. Show your work and put your answer in the table. 1 D 9 3.23916 c. The sea glass has an actual density of 3.50 g/mL. Calculate the percent error. (𝑒𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙 𝑣𝑎𝑙𝑢𝑒−𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒) % 𝑒𝑟𝑟𝑜𝑟 = 𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒 𝑥100 11 0 7 3.23 100 7.71 2. When a rock is thrown into a river, the rock sinks to the bottom. a. Explain why the rock sinks. Rock obtains more density thanwater b. This time the rock is broken in half before being thrown into the river. Will it still sink? Explain. Yesdensity is an intesiveproperty Meaning that splitting therock in half will not effect the fulldensityoftherock PHYSICAL 3. Is density a physical or chemical property? _____________________ 4. Use the graph below to help answer the following questions. a. What does the slope of the line represent? DENSITY _________ b. What is the density of Metal A? (Show your work) 89km c. How many grams of Metal A occupy 5 cm3? Indicate this on the graph with a circle. 41g d. Determine the number of cm3 that will have a mass of 80 g. Indicate this on the graph with a star. 9.9cm e. Water has a density of 1 g/cm3. What is the most likely state of matter for Metal A?_________________ density greater water less SOLID f. Use the table to determine the identity of Metal A. IRON 5. You found a sample of an unknown liquid and took the following measurements: ○ Mass: 5.60 g ○ Volume: 6.35 mL ○ Boiling point: 80.2 ℃ ○ Freezing point: 5.9 ℃ Density 0.88gmL 1 Identify your unknown liquid using the table of known liquid properties. Justify your answer using calculations AND written explanation. Datafor densityboilingpoint attffting point are close to measured values 8 ofthe unknown liquid Unit 2: Matter Elements & Periodic Table; Compounds & Mixtures; States of Matter; Separation Methods; Ideal Gases ELEMENTS & PERIODIC TABLE 1. Annotate the periodic table with the following labels: a. The alkali metals b. The alkaline earth metals c. The transition metals d. The inner transition metals e. The halogens f. The noble gases degases g. Make a key and shade in metals, nonmetals, and metalloids a name ahhhh transition metals ffh 1 Inner transition metals TRUE 2. True or False: Elements in the same group have similar chemical and physical properties. ___________ 3. Identify the following elements, periods, or groups. Period Group Element 4 9 Cobalt co ___________________ 5 ____ 13 ____ Indium, In 1 18 Helium He ___________________ 7 2 Radium Ra ___________________ 4. Circle the pairs of elements listed below that are expected to have similar physical and chemical properties. The first two are given as examples. K and Li Both lithium and potassium are alkali metals, group 1, so they have similar properties. Fe and Na Although iron and sodium are metals, they are not in the same group, so they do not have similar properties. O and N I and Br Mg and Be P and N Ni and Sr 9  5. Describe characteristics of each of the following: a. Metals: Solid at room temp shiny good conductors of heat electricity malleable ductile usually gas at roomtemp dull looking if b. Nonmetals: solid bad conductors of heat electricity brittle if solid c. Metalloids: properties of both metals and nonmetals 6. A student finds a gray chunk on the floor of the chemistry lab. After doing several tests, he discovers that the substance does NOT react with water or acid, it is brittle, and conducts electricity. Is it most likely a metal, metalloid, or nonmetal? Justify your answer. Metalloid has properties ofboth metalsand non metals COMPOUNDS & MIXTURES substances 1. What two categories can matter be divided into? ____________________ and ______________________ mixtures pure elements 2. What two categories can pure substances be divided into? ________________ and ___________________ compounds a. Describe the difference between an element and a compound. Element onlyonetypeofatom of Compund 2types atoms chemically combined 3. Circle the word that correctly completes the sentence: Compounds are (chemical / physical) combinations of two or more different elements. 4. What two categories can mixtures be divided into? ___________________ heterogeneous and _____________________ homogeneous a. Describe the difference between homogeneous and heterogeneous mixtures. Heterogenous of canseedifferentparts the mixture Homogenous entiremixturelooks thesame throughout 5. Circle the word that correctly completes the sentence: Mixtures are (chemical / physical) combinations of two or more pure substances. 10  6. What are the four signs of a chemical change? energychange heatorlight colorchange unexpected gas production bubblessmoke fizzodor of formation precipitate 7. Are changes in state of matter chemical or physical changes? _________________ PHYSICAL 8. Complete the following chart by identifying the type of change and stating why it is that type of change: Change Chemical or Physical WHY? Change melting candle wax physical change in state burning candle wax chemical shell colorchange tearing paper chemical change physical no dissolving NaCl physical no chemicalchange tarnishing chemical color it changed to magnesium reacting with acid baking soda + vinegar fizzing chemical gas made chemical gas made STATES OF MATTER 1. What is matter? anything withvolume and mass 2. What are the 3 states of matter? Describe the shape and volume of each (definite or not definite). a. ____________ solid fixed shape and ____________ : ____________ fixed volume b. ____________ liquid : ____________ variable fixed shape and ____________ volume c. ____________ : ____________ variable shape and ____________ variable volume gas 3. Which state of matter has particles moving at the greatest speed? ______________ gas 4. Which state of matter has the highest energy? ______________ gas solid 5. Which state of matter has particles packed closest together? ______________ solid 6. Which state of matter has the strongest forces of attraction? ______________ 7. What term is defined as the measure of the average kinetic energy of particles? a. Heat c. Noise b. Light d. Temperature 11 8. Outline the main assumptions of the Kinetic Molecular Theory. matterismadeofparticles particlesinteract amountofkineticenergyis measuredbytemp state matter of particles obtainkinetic energy always moving 9. Compare and contrast exothermic and endothermic processes. t.it 1 i t3nanarotnatcmn 10. For the changes in state below, circle the exothermic processes and square the endothermic processes. Sublimation Evaporation Melting Boiling Condensation 000 Freezing Deposition Vaporization 11. Describe what particles of water would look like under the following temperatures: a. The sample is cooled to 0 K. Nokineticenergy particles aren'tmoving b. The sample is cooled to 0 ℃. solidduetofreezingpoint particles arepacked togethervibrating c. The sample is heated to 100 ℃. Gasduetoboilingpoint particlesarespreadout movingrapidly 12. To convert between Kelvin and Celsius, the following equation can be used: K = oC + 273 a. Convert -82 oC into Kelvin. 82 273 160 b. Determine the temperature in oC of a sample that is 39 K. 39 273 23410 13. Annotate the phase change diagram below. Be sure to explain what is happening at each labeled letter as well as the diagonal lines in between the letters. SEEN fullygas TEE.EE solidifies f IIJas sold 12 SEPARATION METHODS 1. Separation methods are _________ techniques to separate ____________. a. physical; compounds c. chemical; compounds 0 b. physical; mixtures d. chemical; mixtures For numbers 2-6, match each separation method to their description. a. Filtration b. Distillation c. Solvation d. Evaporation e. Recrystallization B 2. _____ Separating a liquid mixture based on different boiling points. E 3. _____ Separates a mixture based on differences in solubility at different temperatures. D 4. _____ Separating the solute from the solvent in a highly concentrated solution and being left with a solid form of sugar or salt for example. A 5. _____ Separating mixtures based on particle size for a heterogeneous mixture. C Separates a heterogeneous mixture of two solids; uses both filtration and evaporation during the 6. _____ process. 7. Discuss what you believe to be the most important vocabulary terms to understand when learning about separation methods. Solute us Soluble 8. Write a step-by-step procedure to separate a mixture of salt, water, and sand. Include the physical property utilized in each step. 1 filtration separate sand water 2 evaporation remove IDEAL GASES B 1. _____ At high temperature the particles of a gas: a. Move slower and hit the walls of their container less often O b. Move faster and hit the walls of their container more frequently c. Move slower and hit the walls of their container more frequently d. Don’t move at all and don’t hit the walls of their container 13  B 2. _____ What happens to the volume of a gas during compression? a. The volume increases. O b. The volume decreases. c. The volume remains constant. d. It is impossible to tell because all gases display different behavior. B 3. _____ If the volume of the container holding a gas is tripled while the temperature is held constant, what happens to the pressure of the gas? a. It is tripled O b. It is only one third of the original pressure c. It remains the same d. There is not enough given information. 4. List 2 ways in which real gases may deviate from the behavior of ideal gases. 1 highpressure attractionbetweenparticlescanbeliquid 2 lowtempparticlesmoveslower canbeliquidsolid 5. State the proper units for each of the three factors that affect ideal gases. a. Pressure: kPa b. Temperature: c. Volume: L 6. Describe what the “pressure” of an ideal gas means in terms of its particle behavior. frequencywithparticlesthathitthewalls of container 7. Describe and sketch the graph of the relationships listed below. a. At constant temperature, volume and pressure are ______________ proportional. 8s inversely Volume b. At constant temperature, volume and temperature are ______________ proportional. directly Temperature c. At constant temperature, pressure and temperature are _____________ proportional. directly IS Temperature 14 8. Calculate the unknown in the following scenarios: a. A gas occupies a volume of 4.5 L at a pressure of 108.5 kPa. If the volume is increased to 7.0 L at constant temperature, what will the new pressure be? Given Unknown Equation Solve & Solution Pi 1089 45 P 7.0 Y p py pay 48 29 19 V2 7.0L 71 72 69.79KPat.PL b. A gas at constant pressure occupies a volume of 3.5 L at 350 K. If the temperature is increased to 675 K, what will be the volume of the gas? Given Unknown Equation Solve & Solution 23 6.791 c. A gas has an initial pressure of 107.7 kPa and occupies a volume of 12.0 L. If the pressure is increased to 110.5 kPa and the volume is decreased to 5.0 L, the temperature reaches 250 K. What was the initial temperature? Given Unknown Equation Solve & Solution P107.71Pa Ti R 11077 L.ru 2.21 T is 7 17 76 984.811 15 Unit 3: The Atom Atomic Structure & Subatomic Particles; Isotopes & Average Atomic Mass ATOMIC STRUCTURE & SUBATOMIC PARTICLES 1. The smallest part of an element that can exist and still have the properties of that element is: 0 a. an atom b. an electron c. a proton d. a neutron 2. Complete the following table: Particle Location in Atom Mass in amu Charge How to determine from the (whole number) Periodic Table Proton nucleus 1 atomic Neutron nucleus 0 mass atomic Electron electron atomic cloud 0 1 3. All of the atoms and isotopes of a given element must have the same: a. Number of electrons b. Mass number c. Number of neutrons O d. Number of protons 4. The number of protons in an atom added to the number of neutrons is called: a. The atomic number O b. The mass number c. The atomic mass d. The charge 5. Which subatomic particle contributes the least to the mass of the atom? a. Nucleus b. Neutron c. Proton O d. Electron 6. Label the element’s information below: Periodic Table Symbol Nuclear Symbol atomic mass symbol name atomic 16 average atomicmass  7. Complete the table with the missing information of each neutral atom: Nuclear Atomic Mass Number Number Number Hyphen Notation Notation Number Number of of of Protons Neutrons Electrons 35 17 𝐶𝑙 17 39 17 18 17 Chlorine - 35 IL 3 7 3 4 3 Lithium 7 65 29 𝐶𝑢 29 65 29 36 29 Copper 65 kr 36 85 36 49 36 Krypton 89 58 28 𝑁𝑖 28 58 28 30 28 Nickel 98 ISOTOPES & AVERAGE ATOMIC MASS 1. Atoms which have the same number of protons but different numbers of neutrons are called: a. Ions b. Allotropes c. Isotopes O d. Isomers 2. The weighted average of the masses of all of an element’s naturally-occurring isotopes is called its: a. Mass number b. Atomic mass unit c. Atomic number O d. Average atomic mass 3. What is the difference between average atomic mass on the periodic table and the mass number you find on the nuclear symbol? itiiiit defiled average calculation iiiii 4. Compare and contrast the following isotopes: Carbon-12 and Carbon-13. In 6n 6pt Cartons no 17  5. Calculate the average atomic mass and determine the identity of the element whose isotope and exact atomic masses are listed on the charts below: Mass Number Exact Isotopic % Abundance Decimal Calculation Mass Abundance 10 10.01 19.78% 1978 10.01 1.979978 11 11.01 80.22% 8022 11.01 8 83222 Atomic Mass (to the nearest 0.01): __________ 10.81amu B Symbol of the Element: _______ Mass Number Exact Isotopic % Abundance Decimal Calculation Mass Abundance 32 31.97 95.0% 950 31.97 30.3715 33 32.97 0.76% 0076 32.97 0.290572 34 33.97 4.22% 0422 33.97 1.433934 36 35.97 0.014% 00014 39.97 0.0090358 Atomic Mass (to the nearest 0.01):32.06 __________ amu S Symbol of the Element: _______ Unit 4: Electrons Bohr Model, Electromagnetic Spectrum, Emission Spectra, Orbitals & Energy Levels, Periodic Trends BOHR MODEL & ELECTROMAGNETIC SPECTRUM 1. Draw a Bohr model to represent what happens to an electron when… a. Energy is added b. Energy is released 2. Electromagnetic waves of long wavelength have__________ (high or low) energy. low 3. The higher the energy of a wave, the __________ (greater or lower) the frequency. greater shorter (longer or shorter) the wavelength. 4. The higher the frequency of light, the ___________ red 5. Of the colors of the visible spectrum, which has the lowest energy? ____________ violet 6. Of the colors of the visible spectrum, which has the highest energy? ____________ 18  7. What type of electromagnetic radiation has: a. the highest energy? _______________ gamma ray radio b. the lowest energy? ________________ waves 8. Tell whether the following types of electromagnetic waves have higher or lower energy (frequency) than visible light: lower a. Microwaves _________________ lower b. Radio Waves ________________ c. Ultraviolet ________________ higher d. X-Rays _________________ higher e. lower Infrared ___________________ EMISSION SPECTRA 1. What is the difference between a line emission spectrum and a continuous spectrum? Emission certain 2. What is white light? yyfngthscontinussmktfgyif.fm combined Fyffe all colors on visible spectrum spectrum 3. Explain why we observed different metal ions producing different colors of light when placed in the flame in the flame test lab. tachmetal has different differences levels different amount energy ofenergy wavelength of lightis emitted ORBITALS & ENERGY LEVELS 1. Sketch the orbital shape for each of the following orbitals: s: p: 8 2. A “fuzzy cloud” around the nucleus of an atom where an electron is likely to be found is called: a. an orbital c. ground state O b. valence shell d. none of these 3. The maximum number of electrons that can be located in one orbital is …… a. 1 c. 6 O b. 2 d. 8 4. The sublevel with the lowest energy at any energy level is the O a. b. s p c. d d. f 19  5. Annotate the periodic table below with the main energy levels (1-7) and sublevels (s, p, d, and f). p i d PERIODIC TRENDS f 1. The electrons found in the highest principal energy level or outermost energy level for an atom are called the ______ electrons. These electrons are involved in forming chemical bonds to other elements. O a. b. valence orbital c. excited state d. ground state 2. For each of the following elements, write its number of valence electrons and the charge it acquires when bonding. ve charge ve change Argon 8 ________ ________ 0 Aluminum 3 3 ________ ________ Bromine 7 1 ________ ________ Nitrogen 5 ________ ________ 3 Sodium I ________ 4 ________ Barium ________ 12 2 ________ Potassium I I ________ ________ Helium ________ 0 2 ________ 3. Which elements have complete outer shells? How many valence electrons is this? noble gases 8 2 forHe 4. Which elements have only one valence electron? alkali gases 5. What do you notice about the location (in the periodic table) of the elements in Questions #9 and 10? fullshell last column one we is the firstcolumn 6. Define atomic radius. distance from the nucleus to theoutermost electrons a. Circle the element in each pair with the smaller radius: a) Li or C b) N or P c) Cl or At d) Rb or Y 20 7. Define electronegativity. ability of an atom to attract new elections a. Circle the element in each pair with the smaller electronegativity. a) Li or C b) N or P c) Cl or At d) Rb or Y dec 3 ins 8. Annotate periodic table with arrows to show the periodic trends for: a. atomic size b. electronegativity 21