Trends Handout. Elements with the same number of electron orbitals are found in the. The elements are arranged by increasing.
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1 Trends Handout name: There are 7 trends on the periodic table that we will follow. Using your periodic table, answer all of the questions in the packet. Think hard. The periodic table has groups that go +. The rows that go across left to right are called the. Similar elements are found in. Elements with the same number of electron orbitals are found in the. The elements are arranged by increasing. This is equal to the of and. The ic mass minus the ic number equals the number of. Trend #1 ic mass What is the group trend for ic mass? Why does this trend exist? What is the period trend for ic mass? Why does this trend exist? Explain what happens at the cobalt-nickel part of the table concerning mass and the period trend? Look also at the argon-potassium masses.
2 Trend #2 Atomic Size (the ic radius measured in in pico-meters) Fill in the tables for ic size across period 2, then for groups 2 and 18 below. Li Be B C N O F Ne Radius in pm The Period TREND for ic size/ic radius is Why do s get smaller going across a period? 2 radius in pm 17 radius in pm The Group TREND for ic size or ic radius is... Be Mg Ca Sr F Cl Br Ba I Ra At
3 Trend #3: Nuclear Charge or what is the charge of nucleus of each List the net nuclear charge for Period 2 s below. Then do the same for any 2 groups that you choose. Label WHAT you use, then add symbols and their values. Li Be B C N O F Ne Net Nuclear Charge Describe the TREND for Net Nuclear Charge going across a period. Net Nuclear Charge Net Nuclear Charge Describe the TREND for Net Nuclear Charge going down any group.
4 Trend #4 Electronegativity Define Electronegativity (EN):. Look at Table S, which element has the highest EN value? What is it? Define RELATIVE SCALE:. Fill in this abbreviated Periodic Table, put the EN value for each listed element below its symbol. Fill in the NUMBERS ACROSS THE TOP SET OF EMPTY BOXES H Leave empty He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Ga Ge As Se Br Kr Rb Sr In Sn Sb Te I Cs Ba Tl Pb Bi
5 What is the EN TREND going down a group? What is the EN TREND going across a period? Why do most NOBLE GASES have no Electronegativity value? Which elements of each pair have the higher EN values? (circle higher EN value) Cl or Ca Sr or Ge Br or Cs What is the TREND FOR EN for the whole periodic table? Explain how Xenon and Radon can have an EN value even as noble gases. Explain why group 1 s have lower electronegativity values than the group 17 s. Explain this difference.
6 Trend #5: 1st Ionization Energy Define 1st Ionization Energy: The unit is Fill in this chart with the 1st Ionization Energy levels for each in this chart H Leave empty He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Ga Ge As Se Br Kr Rb Sr In Sn Sb Te I Xe Cs Ba Tl Pb Bi Po At Rn Describe the TREND for 1st Ionization Energy. Define the PERIOD TREND for 1st Ionization Energy. Where are the highest and lowest 1st Ionization Energy values? Why? If you ever forget a TREND, how will you deal with this on the REGENTS?
7 Trend #6: Cation and anion size trends Atom sizes are listed in Table S as ic radius. Cations form when metal s lose electrons, so that they become isoelectric to noble gases. Not only do they lose electrons, they ALWAYS lose all the electrons in the outermost or valence orbital. Cations are ALWAYS smaller than their s. Cations Fill in this chart going down group 2. 2 Be Atomic electron configuration Cation electron configuration It is clear that cations are smaller than their s from this chart. Mg The group trend for cation size is Ca Sr Because Ba Ra Fill in these 2 charts going across period 3 and 4. State the period trend for cation size. Na Mg Al Electron config Cation config K Ca Sc Ti Electron config Cation config
8 Anion Size Anions form when nonmetal s gain enough electrons to fill up the outermost, or valence orbital. They always have the same number of orbitals as the s they form from, but with these extra negative charges all repelling each other, anions are a little bit stretched out as compared to the s they come from. Fill in this chart with the electron configurations of the group 17 s and anions. 17 F Atom electron configuration Anion electron configuration Cl Br I State the group trend for anion size: Fill in this chart for anion size going across period 2 and period 3 N O F Electron config Anion config P S Cl Electron config Anion config State the period trend for anion size:
9 Why are anions always bigger than their s? Trend #7 Metallic Properties + Non-Metallic Properties of the Elements The metals on the table are on the side. The non-metals are on the. Metals properties include: Nonmetal properties include: The most metallic element of them all is. The most non-metallic element of them all is. When comparing, which is most metallic: silver, zirconium, or cesium When comparing, which is most nonmetallic: chlorine, iodine, phosphorous What are metalloids? List the symbols of all the metalloids What are the 2 exceptions to the metalloids?
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Natural Sciences I Lecture 5: Elements and the Periodic Table Classifying MATTER Chapter 0 of your text opens with a discussion of the types of chemical bonds, and also includes a review (pp. 4-4) of the
ANSWER KEY : BUILD AN ATOM PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom )
ANSWER KEY : PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom ) 1. Explore the Build an Atom simulation with your group. As you explore, talk about what
Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model.
John Dalton was an English scientist who lived in the early 1800s. Dalton s atomic theory served as a model for how matter worked. The principles of Dalton s atomic theory are: 1. Elements are made of