The order of decreasing atomic radius is Na, Si, C. This follows the trends in radius. Carbon is the smallest, as it is in period 2, and the rest are in period 3. Period 3 has an additional energy level, making all elements in the period larger. In period 3, atomic radius decreases as you go to the right since the nuclear charge increases as you go to the right. Thus, sodium is larger than silicon.More explanation of the number of energy levels and nuclear charge on valence electron attraction. -1 mark

5.Place the atoms F, N, and P in decreasingorder of ionization energy. Explain your choice of order.The order of decreasing ionization energy is fluorine, nitrogen, phosphorus. Phosphorus is the smallest, as it is in period 3, and the rest are in period 2. The attractive force on the electron is less and less as the number of energy level increases down a column. In period 2, the nuclear charge increases as you go to the right. Thus, fluorine is larger than nitrogen.More explanation of the number of energy levels and nuclear charge on valence electron attraction. -1 mark6.Place the atoms, Cl, F, and Al in decreasingorder of electronegativity. Explain your choice of order.The order of decreasing electronegativity is fluorine, chlorine, aluminum. Chlorine has a higher electronegativity than aluminum as the nuclear charge increases as you go to the right. Chlorine has a lower electronegativity than fluorine as the number of energy levels increases down a column, decreasing the attractiveness for electrons.7.Place the elements Rb, Na, and Mg in order of decreasing chemical reactivity. Explain your choice of order.The order of decreasing chemical reactivity is rubidium, sodium, magnesium. Rubidium is the most reactive as it is period 5 and the rest are in period 3. The outer electrons of metals are easier to

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- Spring '19