Chem Make Up Test

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The elements in this group have electron configurations that end in ns2
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Terms in this set (37)
When calcium becomes an ion it will be isoelectric (have the same electron arrangement as) to a. Potassium (K) b. Argon (Ar) c. Krypton (Kr) d. Neon (Ne)b. Argon (Ar)What is the most active nonmetal (most nonmetallic) in group 7A a. At b. I c. Br d. Cl e. Fe. FWhat is the most active metal (most metallic) in group 1A a. Fr b. K c. Na d. H e. Lia. FrIn periods 4,5 and 6 there is a sharp decrease in the ionization energy between the last transition metal and the first element in group 3A. WHY?The p sublevel is further from the nucleus and higher in energyWhich of the following does not apply to metals a. They make up most of the period table b. They form positive ions c. They have low ionization energies d. They have high electronegatives e. They have low electronegativesdWhy does potassium react at a different rate in water than calcium a. Ca has a larger size and smaller nuclear charge han K b. Ca has fewer electrons to lose than K c. They are in different periods d. Ca has a smaller size and greater nuclear charge than KCa has a smaller size and greater nuclear charge than K dOf the following, which set is arranged in order of increasing ionization energy a. Be, Li, Na (4,3,11) b. C, Si, Ge (6,14,32) c. Si, C, N (14,6,7) d. Mg, Ca, Sr (12,20,38)cOf the following, which set is arranged in order of decreasing electronegativity a. F, Li, Cs (9,3,55) b. N, O, F (7,8,9) c. Se, S, O (34,16,8) d. Na, Li, Be (11,3,4)aWhich of the following would show the greatest increase between the 2nd and 3rd ionization energies a. B(5) b. P(15) c. Ca(20) d. Zn(30)cHigh ionization energies are a characteristic of a. Active metals. b. transition metals c. inner transition metals d. nonmetalsd. nonmetalsOf the follwing, which set is arranged in order of decreasing metallic character a. Ra, Ca, Al (88,20,13) b. O, S, Se (8,16,34) c. Te, Sr, Cs (52,38,55) d. None of thesea. Ra, Ca, Al (88,20,13)What relationship is being shown here and what is the nature of the relationship (direct or inverse)As you move down, the distance from the nucleus increases and the attractive force decreases. Therefore, the nature is inverse.Use this data to explain why pottassium is a bigger atom than sodiumSodium is in the 3rd row and potassium is in the 4th. So, by following this relationship, the distances increases while the attractive force decreases, making K bigger than Na.T OR F Sulfur has a higher first ionization energy than MagnesiumTT OR F Oxygen is more electronegative than chlorineTT OR F Elements within a group are more similar than elements within a periodTSemi-conductor used for computer chipsSi SiliconUnreactive gas for storage of rare documentsNe Neona liquid metal that can be used in electrical switchesGa GalliumAn element that can be used as an insulatorB?Periodic table order A is the smallest of all elements B is the heaviest of all elements C is the most metallic of all elements D is the most nonmetallic of all elements E has an ionization energy that is slightly higher than C, but slightly lower than B F has one electron in its first orbital G has a large just between its 1st and 2nd ionization ernergies H is unreactiveF, A, G, D, H, C, E, BThese are several irregularities in the trends. For example, O actually has a lower ionization energy than N. Why is this? Define IONIZATION ENERGY and then use the diagrams below to help you explain this irregularity. Nitrogen 3p3 Oxygen 3p4Ionization energy is the amount of energy required to move an electron from an atom. O has a lower IE than N because N is more stable than O because a half filled orbital is stable. It would take more energy to remove an electron from N compared to O because O would be fine losing that electron. N, being stable at a half filled orbit, would not want to lose an electron, thus it has a greater ionization energy.What is the trend in electronegativity as you go across a period? What about a group? Explain why.As you go across a period, electronegativity increases because protons are being gained and that has a greater pull on the electrons. You're also approaching non-metals that want to gain electrons, besides noble gases. EN is the tendency of an atom to attract electrons in a chemical bond. As you go down a group, EN decreases because the additional shells make it harder to pull in electrons. Larger atoms have less attraction for electrons because the outer shell is further from the nucleusWhat is the trend in ionization energy as you go across a period? What about down a group? Explain why.As you go across a period, IE increases because smaller atoms have a greater attraction for e-. Because of this, electrons are harder to remove. You're also approaching the nonmetals who want to gain e- to become stable. As you go down a group, IE decreases because larger atoms have less attraction for e- because their outer shell is further from the nucleus. It is easy to remove e- from a large atom.Explain how Mendeleev and Mosely constructed their periodic tables. Name two places where Mendeleev's method did not work.Mendeleev and Mosely both grouped elements with similar properties in the same group. However, their arrangement of elements contrasted, Mendeleev arranged elements in order of atomic mass. Mosely arranged elements by atomic number. Mendeleev's arrangements resulted in several elements being placed in groups of elements with differing properties.Which of the following is a graph of the trend in IE going down a group from Li to Fr? Why? a Up b Down c curved upb. as you go down, the IE decreases because the atom is getting larger, making it easier to lose an electronsDraw bohr model diagrams for the following atoms and ions and list the number of protons and electrons for each. Then rank them from smallest to largest and explain why? Si+4 Na+1 S-2 SSi+4 14p 10e Na+1 11p 10e S-2 16p 18e S 16p 16e Order: SI+4<Na+1<S<S-2 Sl+4 is smaller tha Na+1 because SI+4 has moew protons pulling on the same number of electrons. Na+1 is smaller than S because Na+1 has 1 less shell. S is smaller than S-2 because S-2 has more e- while they both have the same number of protons