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Trends in the Periodic Table I - Atomic and Ionic Radius (Worksheet)
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Name: ______________________________
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Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.
Learning Objectives
- Predict the variation in atomic radius in the periodic table.
- Describe specific reasons for this variation across a period and within a group.
- Predict differences in atomic radius and ionic radius for the same element; predict differences in ionic radius for various oxidation states of the same element.
Many of the trends in the periodic table are useful tools for predicting electronic properties and chemical reactivities of various species, including transition metal complexes. The radius of transition metal ions in inorganic coordination compounds is of great importance in many biologically relevant coordination compounds.
A. Atomic Radius
Critical thinking questions:.
- Write out the complete electron configuration for lithium, sodium, and potassium.
- Write out the complete electron configuration for beryllium, magnesium, and calcium.
- How do the valence electron configurations change as you go from one element to the next in question 1? How do the valence electron configurations change as you go from one element to the next in question 2? How do the complete electron configurations differ from one another for the elements in each of the above questions?
- Predict the trend for the atomic radius for the elements in group I and group II of the periodic table.
- Compare your predictions to the values given in model 1 below.
Model 1: Atomic radii in groups I and II of the periodic table:
1 Slater, J.C., J. Chem. Phys. , 1964, 41 , 3199.
- Write out the complete electron configuration of titanium, and the valence electron configurations of vanadium, chromium, iron, cobalt, arsenic, and selenium. Keep in mind that the electron configuration of some atoms differs from what may be expected.
- How do the complete and/or valence electron configurations change as you go from one element to the next in question 6?
- Going from left to right in period 4 of the periodic table (or any other period), what do you predict the general trend to be for the atomic radius of the elements? Consider the total number of protons and electrons, as well as the valence shell that electrons are added into when going from left to right across a period in your prediction.
- Compare your predictions to the values given in model 2 below.
Model 2: Atomic radii in period 4 of the periodic table:
- Are there any exceptions to the general trends for the atomic radius that can be seen in these models? If so, suggest an explanation for these exceptions.
B. Ionic Radius
- In general, will an anion have a larger or smaller ionic radius compared to the atomic radius of the neutral element that it is derived from? Justify your answer.
- Is the same true for cations? Justify your answer.
- Considering your answer to the previous question, use the information given in model 2 to predict the ionic radius for Fe 2+ , Fe 3+ , V 4+ , and V 5+ .
- Compare your predicted ionic radii from the previous question to values given in the literature.
- Order the ions listed in question 13, as well as V 2+ and V 4+ , in order of increasing size to charge ratio.
- Discuss at least two possible effects that a different size to charge ratio of transition metal ions derived from the same element (e.g. Fe 2+ and Fe 3+ ) could have on properties, reactivities, or chemical behavior of compounds containing inorganic transition metal ions.
- Jens-Uwe Kuhn, Santa Barbara City College
- Jessica Martin, Northeastern State University
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Study with Quizlet and memorize flashcards containing terms like Discuss the importance of Mendeleev's Periodic Law., Identify each element as a metal, metalloid, or nonmetal. a) fluorine b) germanium c) zinc d) phosphorus e) lithium, Give two examples of elements for each category a) noble gases b) halogens c) alkali metals d) alkaline earth metals and more.
Answers to Comparing Ionization Energies. Here are answers to the exercises above. Mg, Si, S All are in the same period and use the same number of energy levels. Mg has the lowest I.E. because it has the lowest effective nuclear charge. S has the highest I.E. because it has the highest effective nuclear charge.
K, P, Br, Na, Fe. 5) Indicate whether the following properties increase or decrease from left to right across the periodic table. a) atomic radius (excluding noble gases) b) ionization energy. c) electronegativity. Periodic Trends Worksheet #3. 1) Rank the following elements by increasing atomic radius: calcium, iron, neon, nitrogen, silicon.
Periodic Trends Worksheet 1. Using the data below, make a bar graph of atomic radius vs. atomic number for Group 2A and for Period 3 of the periodic table. Group 2A Element Atomic Number Atomic Radius Be 4 1.11 Mg 12 1.60 Ca 20 1.97 Sr 38 2.15 Ba 56 2.17 Atomic Number 2. What trends do you notice for the atomic radii of Group 2A?
This page titled 10A: Periodic Trends (Worksheet) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Robert Carter. The size of an atom or ion and the attraction between the nucleus and the outermost electrons play important roles in determining the chemistry of an element.
Periodic trends. Google Classroom. You might need: Periodic table. The first two ionization energies for beryllium are shown below. Be ( g) → Be + ( g) + e − Be + ( g) → Be 2 + ( g) + e − I 1 = 900 kJ/mol I 2 = 1757 kJ/mol. Which of the following identifies the most probable value for the third ionization energy for Be and provides the ...
Microsoft Word - WS 3-3 Periodic Trends.doc. Honors Chemistry. Worksheet 3-3. Name. Periodic Trends Period. 1. Discuss the importance of Mendeleev's periodic law. 2. Identify each element as a metal, metalloid, or nonmetal.
Looking at the elements of the third period gives a good indication of some general trends in the periodic table. The following table shows some physical data for the elements of the third period. Element and symbol. Atomic number. Atomic radius (pm = 10-12 m)
4. Give your best and most concise explanation of the following trends: a) There is a general trend in atomic radius across the table; it decreases as you go from left to right across a period. b) There is a general trend in atomic radius down the table, it increases as you go down a group. 5. Examine the charts above.
The periodic table organizes atoms with similar configurations and properties together in columns. Problem AT6.1. For the following elements, suggest two other elements that would have similar properties. a) zinc, Zn b) calcium, Ca c) oxygen, O d) chlorine, Cl e) chromium, Cr. Problem AT6.2.
5. Circle the atom in each pair that has the largest atomic radius. a) Al B b) S O c) Br Cl. d) Na Al e) O F f) Mg Ca. 6. Put the following elements in order from smallest to largest atomic radius and explain why: C, O, Sn, Sr. ELECTRONEGATIVITY.
Unit 3 exam - AP Chem Prep. Bonding packet 1 - chem. Acid Base Titration Worksheet-calculations including molar concentration and neutralization point. easy trends worksheet and key periodic trends worksheet name using the data below, make bar graph of atomic radius vs. atomic number for group 2a and for period.
Created Date: 11/3/2015 3:20:46 PM
Which element on the periodic table has the highest and lowest electronegativity? Highest electronegativity Lowest electronegativity Ca or Ba Na or K P or Ar Cl or Si Li or K Unit 3 - Periodic Trends: IE, E-neg 2 9. Which element on the periodic table has the most metallic character? 10. Which element on the periodic table has the most non ...
Considering your answer to the previous question, use the information given in model 2 to predict the ionic radius for Fe 2+, Fe 3+, V 4+, and V 5+. Compare your predicted ionic radii from the previous question to values given in the literature. Order the ions listed in question 13, as well as V 2+ and V 4+, in order of increasing size to ...
Study with Quizlet and memorize flashcards containing terms like define electronegativity, Identify each element as a metal, metalloid, or nonmetal. a) fluorine b) germanium c) zinc d) phosphorus e) lithium, Give two examples of elements for each category a) noble gases b) halogens c) alkali metals d) alkaline earth metals and more.
activity you will look at a few periodic trends that can help you make those predictions. Like most trends, they are not perfect, but useful just the same. 1. Consider the data in Model 1 on the following page. a. Each element has three numbers listed under it. ... answer, usin examples from three groups. t,xreaSeS . H K 2 B (33) ( 3. Using ...
The elements calcium and strontium have similar chemical properties because they both have the same. (A) atomic number. (B) mass number. (C) number of valence electrons. (D) number of completely filled sublevels. ____5. On the Periodic Table of the Elements, all the elements within Group 16 have the same number of. (A) valence electrons.
Periodic Trends Worksheet. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table? (A) The number of principal energy levels increases, and the number of valence electrons increases. (B) The number of principal energy levels increases, and the number of valence electrons remains ...
Directions: Use your notes to answer the following questions. 1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium. Oxygen < Carbon < Aluminum < Potassium. 2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. Neon < Aluminum < Sulfur < Oxygen.
6.3 Periodic Trends Section Review Worksheet. atomic radius. Click the card to flip 👆. a. half the distance between the nuclei of two atoms of the same element when the atoms are joined. Click the card to flip 👆. 1 / 6.