Explain how the charge of the metal ions, the number of delocalized electrons and the ionic radius affect the strength of metallic bonding, and account for trends in melting points of s-block and p-block metals down a group and across a period.
Tę umiejętność sprawdza 8 zadań wzorowanych na arkuszach IB z lat 2023–2026.
(i) Describe the structure of solid magnesium and state the forces that hold it together. (ii) Explain why a piece of magnesium can be hammered into a new shape without breaking. (iii) Explain why the melting point of magnesium is higher than that of sodium.
(i) Outline why the strength of the metallic bond increases from potassium, K, to calcium, Ca. (ii) Write an equation for the reaction of potassium, K, with water, including state symbols. (iii) Outline why the electronegativity of chlorine is greater than…
Which list places the metals in order of increasing strength of metallic bonding, from weakest to strongest? A. Rb, K, Sr, Ca B. K, Rb, Ca, Sr C. Sr, Ca, Rb, K D. Ca, Sr, K, Rb
Metallic bonding results from the attraction between a lattice of cations and delocalized electrons. Which of these group 1 metals has the strongest metallic bonding? A. Cs B. Rb C. K D. Na
Which list arranges the metals in order of increasing strength of metallic bonding (weakest first)? A. Rb, Mg, Na, Al B. Al, Mg, Na, Rb C. Rb, Na, Mg, Al D. Na, Rb, Al, Mg
Which of these metals has the strongest metallic bonding? A. Be B. Li C. Na D. Mg
Explain the steady fall in atomic volume from element 11 to element 13.
Magnesium has a higher melting point than sodium. Which statement best explains this? A. Magnesium atoms have a greater relative atomic mass than sodium atoms B. Magnesium has a lower first ionization energy than sodium C. Magnesium ions have a larger radius…
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