1 Chapter 3. Elements, Atoms, Ions, and the Periodic Table The Periodic Law and the Periodic Table In the early 1800's many elements had been discovered and found to have different properties. In 1817 Döbreiner's triads with regularly varying properties: (Mg, Ca, Ba) (F, Cl, Br) and (S Se Te).1865: Newlands "law of octaves", about 55 elements: pattern of reactivity follows after 8 elements. However, no one had found a clear "order" in their properties until Mendeleev, Dmitri ( ) arranged 63 then known elements in the order of increasing atomic mass in a periodic table and showed some chemical properties would reappear periodically. In certain cases, he placed a lighter slightly heavier element before a lighter element so that the chemical properties of the vertical columns would be preserved. Even though in a different and much less clear form Meyer, Lothar ( ) also came up with a graph showing periodic properties similar to Medeleev. In Mendeleev's table, there was a gap. He purposely left blank position in his table so that the consistent vertical columns with the same chemical properties would be preserved. These missing elements were later discovered. The periodic law is an organized "map" of the elements that relates their structure to their chemical and physical properties. The periodic table is the result of the periodic law, and provides the basis for prediction of such properties as relative atomic and ionic size, ionization energy, and electron affinity, as well as metallic or non-metallic character and reactivity. The modern periodic table exists in several forms. The most important variation is in group numbering. The tables in the text use the two most commonly accepted numbering systems. Numbering Groups in the Periodic Table Periods and Groups Periods are the horizontal rows of elements in the periodic table; the columns represent groups or families. Elements in a vertical group have similar chemical properties. The vertical groups are currently named by numbers ranging from 1 to 18. An older way to identify the vertical groups is to use a Roman number and the capital letters A or B. Vertical groups of main group elements (or representative elements) were given a Roman numeral plus the letter A. Vertical groups of transition elements were given a Roman numeral plus the letter B. Representative elements are elements that always lose or gain the same number of electrons in chemical reactions. Transition elements are elements that can lose or gain variable numbers of electrons in chemical reactions. The lanthanide series and the actinide series are parts of periods 6 and 7, respectively, and groups that have been named include the alkali metals, the alkaline earth metals, the halogens, and the noble gases. Group A elements are called representative elements; Group B elements are transition elements. Metals, metalloids, and nonmetals can be identified by their location on the periodic table.
2 These groups are number from 1-18, left to right and groups have their Roman numbers and A or B classification.. Name Elements Common Valence Electron Configuration Group 1 (IA) - Alkali metal: Li, Na, K Rb, Cs, Fr ns 1 Group 2 (IIA) - Alkaline earth metals: Be, Mg, Ca, Sr, Ba, Ra ns 2 Group 13 (IIIA) - No specific name B, Al, Ga, In, Tl ns 2 3p 1 Group 14 (IVA) - No specific name C, Si, Ge, Sn, Pb ns 2 3p 2 Group 15 (VA) - No specific name N, P, As, Sb, Bi ns 2 np 3 Group 16 (VIA) - No specific name O, S, Se, Te, Po ns 2 np 4 Group 17 (VIIA) - Halogens: Cl, Br, I, At ns 2 np 5 Group 18 (VIIIA) - Noble gases: He, Ne, Ar, Kr, Xe, Rn ns 2 np 6 In addition to groups in the periodic table there are three blocks of elements called transition elements (which are labeled with B), Lanthanides and Actinides ( placed bottom of the table. Metals, Nonmetals and Metalloids Most of the elements in the periodic table are metals. Note the stair step line in the periodic table. Elements to the left of the line are metals. Elements to the right of the line are nonmetals. In between metal and non-metals there are semi-metals or metalloids. Metals lose electrons and nonmetals gain electrons. Ionic Compounds are formed when electrons are exchanged in this way between metals and nonmetals. Covalent or Molecular Compounds are formed between non metals and non metals react by sharing electrons. Atomic Number and Atomic Mass The atomic number (Z) of an element represents the number of protons in the nucleus of atoms of that specific element. No two element has that same number of protons. Atomic number after it was discovered proved to be the best order without any discrepancies to arrange the elements in the periodic table and is shown on top of the space for each element. The atomic number will always be a whole number value without decimals. At the bottom average atomic mass calculated based on isotopes of each elements is written.
3 Problem: Pick the a) representative elements, b) transition elements, c) inert gas elements, d) elements that from anions, e) semi- metals, and f) elements that from cations from the following list: Ca, Si, K, Ar, Cu, Fe Zn, Ge, Kr, Cl, O, F. Answer: a) representative elements: Ca, Cl, O, F b) transition elements: Cu, Fe c) inert gas elements: Ar, Kr d) elements that from anions: O, F e) semi- metals: Si, Ge f) elements that from cations: Ca, K, Cu, Fe Zn Look on a periodic chart at the elements listed below. Do you know how to find an elements atomic number? Problem: Use your periodic table to find the symbol, atomic number and atomic mass rounded to two decimal place of each of the following elements: a) Magnesium b) Neon c) Selenium d) Gold Answer Mg, atomic number = 12, mass = amu
4 Ne, atomic number = 10, mass = amu Se, atomic number = 34, mass amu Au, atomic number 79, mass amu Electron Arrangement and the Periodic Table Bohr concluded that the energy levels of an atom can handle only a certain number of electrons at a time. The Quantum Mechanical Atom J. J. Thomson had demonstrated the particle properties of the electron earlier. Because electrons can exhibit diffraction patterns, they have a dual nature of both wave and particle. In 1924, Louis de Broglie suggested that the electron should have wave properties. Light waves exhibit "diffraction." Erwin Schrodinger developed equations to describe the regions around the nucleus where electrons had the probability of being 95% of the time. These regions of high probability for finding an electron around the nucleus were called orbitals. Three dimensional models of the probability regions or orbitals can be constructed. Electron cloud representations are used to show the space that can be occupied by electrons in different energy levels. Building Atoms by Orbital Filling Schrodinger's work showed that each orbital could have a maximum of two electrons. Energy levels could contain different numbers of orbitals. Energy levels further from the nucleus can accommodate more orbitals than energy levels nearer the nucleus. Energy levels can have sublevels when multiple orbitals are present. Orbital Shapes Sub-level Shape # of orbitals/energy level Picture s spherical 1 p dumbbell 3 d complex 5 f very complex 7
5 Energy Levels n=1 n=2 n=3 n=4 number of sublevels one two three four Sublevel Names s s and p s, p and d s. p, d and f Sublevels and orbitals 1s (1) 2s(1) 2p(3) 3s(1) 3p(3) 3d(5) 4s(1) 4p(3) 4d(5) 4f(7) Number orbitals maximum number of electrons per sublevel 2(2n 2 ) 2 + 6= 9(2n 2 ) = 18 (2n 2 ) = 32 (2n 2 ) The maximum number of electrons that can be in an energy level is 2n 2, where n is equal to the energy level being considered. Energy Level maximum number of electrons in an Energy Level # of sublevels Sublevels names n = s 2 n = s, p 2, 6 =8 n = s, p, d 2, 6, 10 =18 n = s, p, d, f 2, 6, 10, 14 =32 Problem: How many electrons are found: Within principle shells? a) n = 1 b) n = 2 c) n = 3 d) n =4 e) n = 5 Answer: a. n = 1; 2n 2 = 2(1) 2 = 2 b. n = 2; 2n 2 = 2(2) 2 = 8 c. n = 3; 2n 2 = 2(3) 2 = 18 d. n = 4; 2n 2 = 2(4) 2 = 32 e. n = 5; 2n 2 = 2(5) 2 = 50 Problem: With in a sub-shells: a) s, b) p c) d, d) f Answer: a) s = 2, b) p=6 c) d=10, d) f= 14 maximum number of electrons per sublevel Problem: With in a Orbital? Answer: Two electrons. Energy Levels and Sublevels A sublevel is a part of a principal energy level and is designated s, p, d, and f. Each sublevel may contain one or more orbitals, regions of space containing a maximum of two electrons with their spins paired. Schrodinger's work showed that Eeach orbital could have a maximum of two electrons. Energy levels could contain different numbers of orbitals. Energy levels further from the nucleus can accommodate more orbitals than energy levels nearer the nucleus.
6 Energy levels can have sublevels when multiple orbitals are present. Building Atoms by Orbital Filling Amazingly, the "electron configurations" of the elements are "embedded" in the Periodic Table. Honk, if you can see this "embedded" information in the Periodic Table? Analogy: The periodic table is actually a packing slip that tells how the electrons are packed around the nucleus. Electronic Configuration - the arrangement of electrons, in orbits or orbitals, around a nucleus of an atom. Electron Configuration and the Aufbau ( Building Up) Principle A scheme used by chemist to obtain electronic configuration of a multi-electron atom in the ground state by filling atomic orbital starting with lowest energy. 1s 2s 2p3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d (building up principle) If two or more orbitals exist at the same energy level, they are degenerate. Do not pair the electrons until you have to.
7 Problem: What is the electron configuration of a) K and b) P? Answer: Using Aufbau principle or periodic table a. Potassium: 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 1 b. Phosphorus: 1s 2, 2s 2, 2p 6, 3s 2, 3p 3 Problem: Examine the electron configurations below, and name the element. 1s 2 2s 2 1s 2 2s 2 2p 3 1s 2 2s 2 2p 6 3s 2 3p 1 Answer: Going through the periodic table. 1s 2 2s 2 (He) 1s 2 2s 2 2p 3 (N) 1s 2 2s 2 2p 6 3s 2 3p 1 (Al) Problem: If a neutral atom in its ground state contains only 5 electrons in its outermost p sublevel, it is an atom in what "vertical group" of elements? Answer: group 17 or VIIB or Halogen family. Problem: If a neutral atom in its ground state contains 2 electrons in its outermost s sublevel, it is an atom in what "vertical group" of elements? Answer: group 2 or IIA or Alkaline Earth family. Problem: State what is similar and what is different about the electron configuration of fluorine and chlorine. Answer: F: 1s 2 2s 2 2p 5 Cl: 1s 2 2s 2 2p 6 3s 2 3p 5 valance shell electron configuration is similar but electron configurations are different. Problem: Fluorine and chlorine have similar chemical properties. Oxygen and sulfur have similar chemical properties. However, oxygen and sulfur have chemical properties different from fluorine and chlorine. What does electron configuration have to do with this observation? Answer: F: 1s 2 2s 2 2p 5 Cl: 1s 2 2s 2 2p 6 3s 2 3p 5 both have same vala.nce electron configurations and similar chemical properties. O: 1s 2 2s 2 2p 4 S: 1s 2 2s 2 2p 6 3s 2 3p 4 both have same valance electron configurations and similar chemical properties.. However, two groups F, Cl: ns 2 np 5 and O, S: ns 2 np 4 have different valance electron configurations creating different chemical properties. Valence Electrons The outermost electrons in an atom are valence electrons. For representative elements, the number of valence electrons in an atom corresponds to the group or family number. If atoms of different elements have the same electron arrangement in their valence shell electrons, then they can have similar chemical properties even if their atomic numbers or atomic masses are quite different. Metals tend to have fewer valence electrons than nonmetals. Valence electrons are involved in chemical interactions and bonding (valence comes from the Latin valere, "to be strong"). Valence shell electrons are available to be lost, gained, or shared in chemical reactions. Problem: How many total electrons and valance electrons are in the following atoms: a) K, b) F, c) P, d) O and e) Ca Answer For counting valance electrons go to the period the element is found and count ( excluding transition element blocks) from left to right until element is found. a. Total electrons = 19 (same as atomic number), valence electrons = 1 b. Total electrons = 9 (same as atomic number), valence electrons = 7 c. Total electrons = 15 (same as atomic number), valence electrons = 5 d. Total electrons = 8 (same as atomic number), valence electrons = 6
8 e. Total electrons = 20 (same as atomic number), valence electrons = 2 Abbreviated Electron Configurations Abbreviated electronic configuration is separating valance electrons from core electrons and designating core electrons as a noble gas. E.g. What is the abbreviated electron configurations of a) K, b) P and Sn? Answer First, obtain the electron configuration then find the valence electrons. a. Potassium (K): 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 1 b. Phosphorus (P): 1s 2, 2s 2, 2p 6, 3s 2, 3p 3 c. Tin (Sn): 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6, 5s 2, 4d 10, 5p 2 Second, lump all non valance electrons as core abbreviated as a noble gas con figuration. a. Ar: 1s 2, 2s 2, 2p 6, 3s 2, 3p 6 = [Ar] b. Ne: 1s 2, 2s 2, 2p 6, 3s 2 = [Ne] c. Kr: 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6 = [Kr] Final answer a. Potassium (K): [Ar] 4s 1 b. Phosphorous (P): [Ne] 3s 2, 3p 3 c. Tin (Sn): [Kr] 5s 2, 4d 10, 5p 2 Electron configuration of the elements is predictable, using the Aufbau Principle. Knowing the electron configuration, we can identify valence electrons and begin to predict the kinds of reactions that the elements will undergo. Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all have a complete outer shell. An atom chemically reacts to fill its valance shell. A full valance shell contains eight electrons there fore the name octet. The octet rule tells us that in chemical reactions atoms of elements will gain, lose or share the minimum number of electrons necessary to achieve the electron configuration of the nearest noble gas. octet rule - the rule which predicts that atoms form the most stable molecules or ions when they are surrounded by eight electrons in their highest occupied energy (valance) level. Electronic configuration of ions Series of negative ions, noble gas atom, and positive ions with the same number electrons and electronic configuration. Electron configuration of ions is obtained by adding more electrons (anions) or removing electrons (cations) from a neutral atom. In the process atoms achieves a noble gas electron configuration. Group 1 (or IA), Alkali Metals have one valence electron. They all form +1 cations when the single valence electron is lost. Metals lose electrons and achieve electron configuration of preceding noble gas. E.g. Potassium (K): K K + (cation) + e - Oxygen (O):
9 O + 2e - O 2- (anion) Metallic elements tend to form cations and nonmetals form anions that are isoelectronic with their nearest noble gas neighbor. Isoelectronic electronic configurations If atom and a cation or anion have same number of electrons they are called isoelectronic. E.g. K + and Ar O 2- and Ne Problem: Which of the following are isoelectronic: F,Cl, K +, Ar Answer: a. F, 10e ; Cl, 18 e ; Not isoelectronic b. K +, 18 e ; Ar, 18e ; Isoelectronic Ion Formation and the Octet Rule Metals lose electrons and achieve a an octet of valance electrons similar to electron configuration of preceding noble gas. E.g. Potassium (K): [Ar] 4s 1 K ([Ar] 4s 1 ) K + ([Ar]) + e - Oxygen (O): [He] 2s 2 2p 4 O ([He] 2s 2 2p 4 ) + 2e - O 2- ([Ne]) a. I (54 e ) = Xe= 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6, 5s 2, 4d 10, 5p 6 b. Ba 2+ (54 e )= Xe= 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6, 5s 2, 4d 10, 5p 6 c. Se 2 (36 e ) =Kr = 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 6 d. Al 3+ (10 e )=Ne = 1s 2, 2s 2, 2p 6 Trends in the Periodic Table Atomic Size Atomic size increases from top to bottom but decreases from left to right in the periodic table. Cations are smaller than the parent atom. Anions are larger than the parent atom. Ions with multiple positive charge are even smaller than their corresponding monopositive ion; ions with multiple negative charge are larger than their corresponding less negative ion. Problem: Arrange the following list of elements in order of increasing atomic size. a) Al, Si, P, Cl, S b) In, Ga, Al, B, Tl c) Sr, Ca, Ba, Mg, Be d) O,N, Sb, Bi, As Answer: a. (Smallest) Cl, S, P, Si, Al (Largest) b. (Smallest) B, Al, Ga, In, Tl ( Largest) c. (Smallest) Be, Mg, Ca, Sr, Ba (Largest) d. (Smallest) N, P, As, Sb, Bi (Largest) Ionization Energy The energy required to remove an electron from an atom in the gas phase.
10 The energy required to remove an electron from the atom is the ionization energy. Descending a group, the ionization energy decreases. Proceeding across a period, the ionization energy increases. Problem: Arrange the following list of elements in order of increasing ionization energy. a) N,F, O b) Li, K, Cs c) Br, I, Cl Answer: a) (Smallest) N, O, F(Largest) b) (Smallest) Cs, K, Li (largest) d) (Smallest) Cl, Br, I (Largest) Electron Affinity The energy released when a single electron is added to neutral atom in the gaseous state is known as the electron affinity. Electron affinities generally decrease proceeding down a group and increase proceeding across a period. Exceptions exist for periodic trends. They are generally small anomalies, and do not detract from the predictive power of the periodic table. Problem: Arrange the following list of elements in order of increasing ionization energy. a. Na, Li, K b. Br, F, Cl c. S, O, Se Answer: a. (Smallest) Li, Na, K (Largest) b. (Smallest) F, Br, Cl (Largest) c. (Smallest) Se, S, O (Largest) Ion Size Ions follows same trends as for atomic radius in a group, fro example taking oxide and sulfide ion: radius of O 2- < S 2-. Cation or positive ions have fewer electrons than neutral atom and nuclear charge being same attract remaining electrons strongly making cation smaller than the neutral atom Anions or negative ions larger than neutral atom. Anions are larger than the atoms from which there are formed. Adding electrons to an atom increases the repulsion between electrons. Anion has a harder time holding on to the electrons.
11 CHEM 120 Homework 3. Chapter 3 1. In the modern periodic table, the elements are arranged according to increasing. a. atomic masses b. number of neutrons c. atomic number d. mass number 2. How many periods are found on the periodic table? a. 2 b. 7 c. 18 d Which period contains the element Cesium? a. 2 b. 4 c. 6 d Where are the alkaline earth metals located on the periodic table? a. Group 1 (IA) b. Group 2 (IIA) c. Group 13 (IIIA) d. Group 14 (IVA) e. Group 17 (VIIA) 5. Which one of the following is not a representative element a. Na b. As c. Ca d. Fe e. Cl 6. How many orbitals are in an s sublevel? How many in a p sublevel? a. 2;6 b. 1;1 c. 1; 3 d. 3; 5 7. Which of the following correctly gives the electron capacity of a principal energy level in terms of the number n? a. n b. 2n c. 2n + 2 d. n 2 e. 2n 2 7. What requirement must be met in order for two electrons to coexist in the same orbital? a. they go to a s orbital b. they go to a p orbital c. they must have opposite spins d. they must have parallel spins 8. How many valence electrons are present in an atom of silicon? a. 2 b. 3 c. 4 d. 5 e The electronic configuration in an atom of argon, a. 1s 2 2s 2 b. 1s 2 2s 2 2p 6 c. 1s 2 2s 2 2p 6 3s 2 3p 6 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p Common valence electron configuration of halogens a. ns 1 b. ns 2 c. ns 2 3p 2 d. ns 2 np 3 e. ns 2 np What is not isoelectronic with K +? a. S 2- b. Ar c. Cl - d. Na + e. Ca Which of the following atoms has the biggest size (radius)? a. Na b. Al c. Cl d. Rb e. I 13. Which of the following elements has the highest ionization energy? a. Li b. B c. O d. F e. Ne 14. Which one of the following elements has the highest electron affinity? a. Li b. K c. Kr d. O e. Cl 15. What charge is found on a ion from Al? a. +1 b. -2 c. +3 d. -3
12 Sample Test Chapter 3 1. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements? Ans. Mendeleev and Meyer 2. Who stated that the elements, when arranged according to their atomic masses, showed a distinct periodicity of their properties? Ans. Dimitri Mendeleev 3. In the modern periodic table, the elements are arranged according to what system? Ans. increasing atomic number 4. The modern periodic law states that the physical and chemical properties of the elements are periodic functions of what property? Ans. atomic number 5. What do we call the horizontal row of elements on the periodic table? Ans. periods 6. How many periods are found on the periodic table? Ans. seven 7. Which period contains the element sodium? Ans. three 8. What do we call the columns of elements on the periodic table? Ans. groups 9. What number for an atom gives the number of electrons and protons found in that atom? Ans. atomic number 10. Where are the alkaline earth metals located on the periodic table? Ans. Group IIA (2) 11. What is the general name given to the elements of Group VIIA (17)? Ans. Halogens 12. What term is used for the elements straddling the "staircase" boundary between the metals and nonmetals? Ans. Metalloids or semi-metals 13. For a representative element, how can we deduce the number of valence electrons in a neutral atom from the position of the element in the Periodic Table? Ans. the group number (Roman numbers with Bs) is also the number of valence electrons 14. How many orbitals are in an s sublevel? How many in a p sublevel? Ans, 1; In what way(s) are the three orbitals in the 2p sublevel similar; in what way(s) are they different? Ans. they have the same shape and the same energy; they are oriented differently in space 16. What requirement must be met in order for two electrons to coexist in the same orbital? Ans. they must have opposite spins 17. State the Aufbau Principle. Ans. Electrons occupy the available orbital of lowest energy first. 18. How many electrons are present in an atom of silicon? Ans. Fourteen 19. Give the electronic configuration in an atom of argon, element number 18. Ans. 1s22s22p63s23p6 20. Give the electronic arrangement in an atom of strontium, element number 38. Ans. 1s22s22p63s23p64s23d104p65s2 21. How many electrons are present in a chloride ion? Ans. Eighteen 22. State the Octet Rule. Ans. Elements tend to react in such a way as to attain the electron configuration of the atoms of the noble gas nearest to them in the Periodic Table 23. Give the name of a Group IA (1) ion that has the following electronic arrangement: 1s 2 2s 2 2p 6 Ans. sodium ion 24. Give the name of a VIIA (17) ion that has the following electronic arrangement: 1s22s22p63s23p6 Ans. chloride 25. What ion carries a 2- charge and is isoelectronic with K +?
13 Ans. S Give the complete electronic arrangement of a sulfide ion, S 2-. Ans. 1s22s22p63s23p6 27. Atoms with the biggest radii occur in the region of the Periodic Table. Ans. bottom left 28. How would you expect an Al 3+ ion to compare in size with an Al atom? Explain why? Ans. The ion will be much smaller. In forming the ion, the atom loses all its outermost electrons. The net positive charge on the ion ensures that all the electrons in the ion are strongly attracted to the nucleus, keeping the ion small. 29. Which group of elements has the highest ionization energies? Which group has the lowest? Ans. Group VIIIA (18) are highest; Group IA (1) are the lowest. 30. Explain what is meant by electron affinity. Ans. It is the energy released when a neutral atom gains an electron to form an anion. 31. In Mendeleev's table of the elements, they were arranged according to A. atomic number B. mass number C. atomic mass D. neutron number E. density Ans. C. atomic mass 32. The modern periodic table is arranged according to what property? A. atomic number B. mass number C. atomic mass D. neutron number E. density Ans. A. atomic number 33. What do we call a complete horizontal row of elements on the periodic table? A. group B. period C. family D. representative elements E. transition elements Ans, B 34. What are all the elements in the A-groups often called? A. transition elements B. lanthanides C. metals D. non-metals E. representative elements Ans. E 35. Which of the following elements is a metalloid? A. C B. Ge C. Pb D. N E. P Ans. B 36. Where are the alkali metals located on the periodic table? A. representative elements B. transition metals C. Group IA (1) D. Group IIA (2) E. Group IIIA (3) Ans. C 37. How many valence electrons are in an atom of carbon? A.8 B. 6 C. 4 D. 1 E. 0 Ans. C 38. What is the lowest energy sublevel of a principal level? A. d B. e C. f D. s E. p Ans. D 39. How many sublevels are there in the third principal energy level? A. 3 B. 2 C. 1 D. 0 E. 4 Ans. A 40. How many orbitals are there in a p sublevel? A. 2 B. 3 C. 1 D. 0 E. 4 Ans. B 41. Which of the following correctly gives the electron capacity of a principal energy level in terms of the number n? A. n B. 2n C. 2n + 2 D. n 2 E. 2n 2 Ans. E 42. What is the electron configuration of sulfur, atomic number 16? A. 1s 2 1p 6 2s 2 2p 6 B. 1s22s22p62d6 C. 1s22s22p63s23p4 D. 1s22s22p63s23d4 E. 1s22s22p63s22d4 Ans. C 43. Which one of the following electron configurations is appropriate for a normal atom? A. 1s12s1 B. 1s22s1 C. 1s22s22p8 D. 1s22s22p43s1 E. 1s22s22p63d1 Ans. B
14 44. Which of the following elements is most likely to form a 3+ ion? A. Li B. K C. Al D. N E. Cu Ans. C 45. Give the complete electronic configuration of a sodium ion. A. 1s22s22p5 B. 1s22s22p6 C. 1s22s22p63s1 D. 1s22s22p63s2 E. 1s22s22p63s23p64s1 Ans. B 46. Which of the following ions does not follow the octet rule? A. Na+ B. Ca2+ C. Al3+ D. N3- E. Cl2- Ans. E 47. Which of the following atoms has the biggest size (radius)? A. Na B. Al C. Cl D. Rb E. I Ans. D 48. Which of the following elements has the highest ionization energy? A. Li B. B C. O D. F E. Ne Ans. E 49. Which of the following elements has the lowest ionization energy? A. Li B. B C. O D. F E. Ne Ans. A 50. The electron affinity is A. the energy required to remove an electron from an isolated atom B. the force between two electrons in the same orbital C. the force between two ions of opposite charge D. the energy released when an isolated atom gains an electron E. the attraction of an atom for an electron in a chemical bond Ans. D 51. Which one of the following elements has the highest electron affinity? A. Li B. K C. Kr D. O E. Cl Ans. E 52. T F In Mendeleev's table, the elements were arranged according to their atomic numbers. Ans. F 53. T F There are nine periods on the periodic table. Ans. F 54. T F Sulfur (S) is one of the representative elements. Ans. T 55. T F Platinum (Pt) is a lanthanide element. Ans. F 56. T F Tin (Sn) is a metalloid. Ans. F 57. T F Valence electrons are involved when atoms form bonds. Ans. T 58. T F There are a maximum of 50 electrons in principal energy level number five. Ans. T 59. T F Atoms of the noble gas elements, Group VIII A (18), do not form bonds with any other elements. Ans. F 60. T F There are eight valence electrons in a chloride ion. Ans. F 61. T F The ions formed from Group IIA (2) atoms have charges of 2+. Ans. T 62. T F Cations tend to be formed from metal atoms, while anions are formed from non-metal atoms. Ans. T 63. T F The atoms of smallest radius are those of elements in top left hand part of the periodic table. Ans. F 64. T F The halogens (Group VII A (17)) have the lowest ionization energies of any group in the periodic table.
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Language of Chemistry includes chemical symbols of elements, chemical formulas, & chemical equations All known elements (ca.100) are arranged in Periodic Table. Sodium Na Potassium K Hydrogen H Each element
CHEM100 Week 4 Notes Page 1 of 6 Scientists create models to understand how things work, including atoms. Dalton created a theory for the atom with these 5 postulates 1. Elements consist of one or more
PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06
CLASS: X NCERT (CBSE) Chemistry: For Class 10 Page : 1 Question 1: Explain 'Dobereiner's Triads and its drawback. Dobereiner classified elements into groups of three where the atomic weight of the middle
Worksheet 11 - Periodic Trends A number of physical and chemical properties of elements can be predicted from their position in the Periodic Table. Among these properties are Ionization Energy, Electron
Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You
CHEMISTRY TEST: THE PERIODIC TABLE Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet. 1. Which of the following
Chapter -9 Classification of Elements The periodic Table SYNOPSIS From the earliest times, scientists have been trying to classify the available elements on the basis of their properties. Dobereiner proposed
.0 Elements, Symbols and Periodic Table Dr. Fred O. Garces Chemistry 00 Miramar College.0 Elements, symbols and the Periodic Table January 0 The Elements: Building block of Matter The periodic table of
The Periodic Table Organizing the Elements A few elements, such as gold and copper, have been known for thousands of years - since ancient times Yet, only about 13 had been identified by the year 1700.
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
Chapter 6. Periodic Relationships Among the Elements Student: 1. The nineteenth century chemists arranged elements in the periodic table according to increasing A. atomic number. B. number of electrons.
Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06 (B) 1.95 (C) 13.5 (D) 18.7 (E) 208 2. Which peak corresponds to the valence 3p orbital?
CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek
TEST NAME: Chemistry ES 1.3 TEST ID: 61960 GRADE:11 SUBJECT:Life and Physical Sciences TEST CATEGORY: My Classroom Chemistry ES 1.3 Page 1 of 10 Student: Class: Date: 1. The electron configuration of an
Periodicity and the Periodic Table the result Dmitri Mendeleev arranged elements in order of their atomic numbers, such that elements with similar properties fell into the same column or group. The Periodic
The Periodic Table: Chapter Problems Periodic Table 1. As you move from left to right across the periodic table, how does atomic number change? 2. What element is located in period 3, group 13? 3. What
1. Which characteristics describe most nonmetals in the solid phase? (1) They are malleable and have metallic luster. (2) They are malleable and lack metallic luster. (3) They are brittle and have metallic
68 Blocks on the periodic table 11 Sodium 22.99 Atomic number: This is always a whole number. The periodic table is arranged by atomic number! Element symbol: A one or two letter abbreviation for the name
Chemistry: The Periodic Table and Periodicity Name: per: Date:. 1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What
Atomic Structure and the Periodic Table Chapter 3 Chemistry 104 Professor Michael Russell Atomic Theory Chemistry founded on four fundamental assumptions about atoms and matter which make up the modern
Name Period Date Honors Chemistry - Periodic Trends Check Your Understanding Answer the following, formulating responses in your own words. (This helps you better understand the concepts) 1. Define shielding
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.
Chemistry: The Periodic Table and Periodicity Name: Hour: Date: Directions: Answer each of the following questions. You need not use complete sentences. 1. Who first published the classification of the
Question Bank Periodic Table and Periodic Properties 1. Name the following with reference to the elements of Modern Periodic Table. (1 26) (a) An alkali metal in period 2. Ans. Lithium (b) A halogen in
Chemistry - Elements Electron Configurations The Periodic Table Ron Robertson History of Chemistry Before 16 th Century Alchemy Attempts (scientific or otherwise) to change cheap metals into gold no real
Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based
Chemistry Unit 5- Periodic Table and Periodic Law Name: History of the Periodic Table I. Mendeleev and Chemical Periodicity A. Wanted to organize elements according to their B. When elements were arranged
Name: Class: Date: ID: A Unit 7 Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1) In which set of elements would all members be expected to have very
3.06 Periodic Table and Periodic Trends Dr. Fred Omega Garces Chemistry 100, Miramar College 1 3.06 Periodic Table and Periodic Trend The Periodic Table and the Elements What is the periodic table? What
Unit 5 Elements and their Properties 1. In 1871, Russian chemist Mendeleev created the forerunner of the modern periodic table. 2. The elements in Mendeleev's table were arranged in order of increasing
EXPERIMENT 4 The Periodic Table - Atoms and Elements INTRODUCTION Primary substances, called elements, build all the materials around you. There are more than 109 different elements known today. The elements
1 Ch 3 Atomic Structure and the Periodic Table Figure 3.1 size relationship is not to scale, ratio of average diameters atom/nucleus = 10 5 2 Atoms are very small and spherical. Radii Range 0.9 x 10-10
Name Date STUDY GUIDE CHAPTER 1 ATOMS AND ELEMENTS 1) DESCRIBE THE RUTHERFORD-BOHR ATOMIC MODEL All matter is made of small particles called atoms. An atom is the smallest unit of matter that retains the
5.4 Trends in the Periodic Table Think about all the things that change over time or in a predictable way. For example, the size of the computer has continually decreased over time. You may become more
DEVELOPMENT OF THE PERIODIC TABLE Prior to the 1700s, relatively few element were known, and consisted mostly of metals used for coinage, jewelry and weapons. From early 1700s to mid-1800s, chemists discovered
1. 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
3 Classification of Elements and Periodicity in Properties 1. Which of the following statement is not correct for the element having electronic configuration 1s 2 2s 2 2p 6 3s 2 (a) It is a divalent electropositive
Atoms and Elements 2 Answers and Solutions to Text Problems 2.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 2.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 2.3 a. carbon b. chlorine c. iodine d. mercury
179 ELECTRON CONFIGURATION (SHORT FORM) - We can represent the electron configuration without drawing a diagram or writing down pages of quantum numbers every time. We write the "electron configuration".
Electron Configurations, Isoelectronic Elements, & Ionization Reactions Chemistry 11 Note: Of the 3 subatomic particles, the electron plays the greatest role in determining the physical and chemical properties
The Periodic Table of The Elements Elements are like a collection As more and more elements were discovered it became more important to organize and classify them Between the late 1700 s and mid 1800 s
Periodic Table Trends in Element Properties Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\ch9trans2.doc The Periodic Table Quick Historical Review Mendeleev in 1850 put together
Unit 6 Particles with Internal Structure 3-1 The Elements Remember, elements are combined to form molecules the way letters are combined to form words. Presently there are about 115 known elements. Only
PERIODIC TABLE OF ELEMENTS, a Russian scientist is credited with creating the periodic table. Periods tell us how many are in the atoms of each element. Groups help us to know how many electrons are in
The Periodic Table Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations. Vertical Rows are called Families or Groups.
Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.
6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification
UNIT-3 Classification of elements and periodicity in properties One mark questions:. For the triad of elements A, B and C if the atomic weights of A and C are 7 and 39. Predict the atomic weight of B..
Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core
Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has
Reading Guide - Chapter 8.1 Periodic Properties of the Elements Section 1 - Main Group Elements Patterns of Behavior of Main Group Elements (Groups 1, 2, and 13-18) 1. Elements in the same group have the
Key Concepts: Periodic Properties of the Elements 1. Understand and be able to predict and explain trends in effective nuclear charge, Z eff. 2. Understand and be able to predict and explain the periodic
Review- The Periodic Table Name Date Block Matching: Match the description in with the correct term in. Write the letter in the blank provided. Each term matches with only one description, so be sure to
Some Basic Concepts & Classification of Elements Test No. 15 Time: 2 Hrs. Total Marks: 311 Date: 07/07/2013 Name Batch: CLASSIFICATION OF ELEMENTS Section A (Objective Question only one correct answer)
1. Structure and Properties of the Atom 1.1 Atoms: A simple definition of the atom is that it is the smallest particle that contains the properties of that element. The idea of atoms was first suggested
CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered
Date: Science 10 4.1 Atomic Theory & Bonding What is an Atom? smallest particle of an element that still has the properties of that element An atom = proton(s) + electron(s) + neutron(s) (PEN) Fun Fact:
Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the
Periodic Table Extra Practice 1. Which of the following elements in Period 3 has the greatest metallic character? 1) Ar 3) Mg 2) Si 4) S 2. Which sequence of atomic numbers represents elements which have
Material: laboratory display of the elements and a wall periodic table is required. Objective: To learn the use of periodic table for writing electron configuration of elements. INTRODUCTION Basic building
Noble gases Period alogens Alkaline earth metals Alkali metals TRENDS IN TE PERIDI TABLE Usual charge +1 + +3-3 - -1 Number of Valence e - s 1 3 4 5 6 7 Electron dot diagram X X X X X X X X X 8 Group 1
1. The atomic number of an atom is always equal to the total number of A. neutrons in the nucleus B. protons in the nucleus 2. All of the atoms of argon have the same A. mass number B. atomic number C.
Question (1) Chapter Two Periodic Table Choose the correct answer for each statement of the following:- 1- The elements of same vertical group are identical in the number of----------- a valence electrons