![]() X is a nonmetal because it contains fluorine and it creates an anion. X + 2F2 → XF4 An element X reacts with F2(g) to form the molecular product shown here.ĭo you think that X is a metal or nonmetal? Nonmetal Write a balanced equation for this reaction (do not worry about the phases for X and the product). An element X reacts with F2(g) to form the molecular product shown here. How are common oxidation states divided by this line? Anions are above the line cations are below the line. The red stepped line divides metals from nonmetals. ![]() If you were told that AA is either scandium or phosphorus, which do you think is the more likely choice? PCl3 How do the periodic trends in metallic character compare to those for ionization energy? Metals tend to have lower ionization energies than nonmetals. ![]() Would you expect the compound to be molecular or ionic? Molecular A compound ACl3 (A is an element) has a melting point of -112 ∘C. A compound ACl3 (A is an element) has a melting point of -112 ∘C. Sb Which is not a characteristic of metals? They are poor conductors of heat and electricity. Which of the following correctly lists nonmetals that exist under ordinary conditions as diatomic molecules? Cl, Br, F, O Metalloids have properties intermediate between those of metals and nonmetals. Ordering these elements by the electron affinity provides an identical order:į>O>C>Li>Be Why are the electron affinities of the Group 4A elements more negative than those of the Group 5A elements? Group 5A half-filled pp-subshells discourage addition of an electron. The tendency to gain an electron is quantitatively measured by the electron affinity, the amount of energy involved in the addition of an electron to a neutral gaseous atom. Arrange the elements S, P, Cl, and Ca in order of increasing electronic affinity (EA). Which of the following correctly describes the measurement of an atom's electron affinity? It measures the ease with which an atom gains an electron. When looking at a series of atoms within the same period, the greater the pull on the electrons, the smaller the atom and the harder it is to remove an electron. The inward "pull" on the electrons from the nucleus is called the effective nuclear charge. Se, Ge, In, Cs For the series of elements XX, YY, and ZZ all in the same period (row), arrange the elements in order of decreasing first ionization energy.ĮlementRadius(pm)X124 Y 179 Z 257 Highest -> Lowest Which of the following shows a correct relationship between first ionization energies of the given atoms? Ne > F What is the ground state electronic configuration of Ti+4? What is the ground-state electron configuration of a neutral atom of nickel? 3d^84s^2 What is the ground-state electron configuration of the chloride ion Cl−? Which element has the following configuration: 6s^24f^4? Nd Arrange the elements in decreasing order of first ionization energy. The red sphere represents a metal because it loses electrons in the reaction and turns into a cation. Largest -> Smallestī, C, H Which sphere represents a metal and which a nonmetal? Red sphere represents a metal, the blue sphere represents a nonmetal. Rank elements from largest atomic radius to smallest atomic radius. ![]() Which part of the periodic table has the elements with the largest atoms? bottom and left Na, Ra, and Sr: Therefore, the electrons in oxygen are held closer to the nucleus, giving it a smaller radius. The valence electrons in an oxygen atom are attracted to the nucleus by a positive charge nearly double that of boron. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively? +3 and +6 Largest -> Smallest Si, P, S, Cl The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Rank the following elements in order of decreasing atomic radius.
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