Presentation top top theme: "Chemistry Homework review pp. 132-141 problems p. 141 #1,2,3,5,10,12,13,14."— Presentation transcript:




You are watching: Why is measuring the size of an atom difficult

1 Chemistry Homework review pp. 132-141 problems p. 141 #1,2,3,5,10,12,13,14

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2 1.What is ionization energy? A: (p. 133) Ionization power is the power required to remove an electron from an atom or ion. Note: number 16 ~ above p. 133 shows the ionization that lithium. The snapshot below reflects the ionization that sodium. Both reactions call for some lot of ionization energy.

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3 2. Why is measure the dimension of one atom difficult? A: (p. 135) one atom’s size relies on the volume (amount the space) the electrons take up about the nucleus. The electron cloud has no clean edge. Also, the dimension of the electron cloud can adjust based ~ above the chemical and physical environment. Notes: number 19 top top p. 135 shows exactly how atomic radius is measured.

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4 3. What have the right to you tell around an atom that has actually high electronegativity? A: (p. 137) Atoms through high electronegativity pull electrons towards them an ext than atoms v low electronegativity. Notes: number 22 and 23 display the fads for electronegativity. In the snapshot below, the Oxygen (O) is more electronegative (pulls harder on electrons) than Hydrogen (H).

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5 5. What routine trends exist for ionization energy? A: (p. 133-134) Ionization energy decreases together you relocate down a group. Ionization energy increases together you move throughout a duration from left come right. Notes: number 17 and 18 present the ionization power trends. Compare the chart below to number 17. Execute they present the same trend?

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6 10. What periodic trends exist for electronegativity? A: (p. 137-138) Electronegativity decreases together you move down a group. Electronegativity increases as friend move across a duration from left come right. Notes: figure 22 and 23 display the ionization energy trends. To compare the chart below to number 22. Execute they present the exact same trend? to compare to the ionization power trend.

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7 12. Describe why the noble gases have high ionization energies. A: (p. 134) The noble gases have high ionization energies because their outer electron covering (energy level) is full. This is a stable state and it takes a many of power to do an atom unstable. Also, in compare to other atoms in the same period, noble gases have the maximum variety of protons pulling on electrons that are a similar distance away from the nucleus. Notes: The second paragraph ~ above p. 134 defines this idea.

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8 13. What do you think happens to the size of an atom when the atom loses an electron? Explain. A: (p. 136, 139) The atom’s radius decreases. The size of the atom it s okay smaller. Once an electron is taken far the atom i do not care a positively charged ion. There are more protons 보다 electrons. This uneven hopeful charge traction the negatively fee electrons that space left closer come the nucleus. Also, if the electron that was taken to be the just one in the outer power level, over there is bigger decrease in size because there space less power levels. Notes: To number this out, incorporate the discussion about decreasing atom radius going across a duration with the discussion around ionic radius. Number 16 also helps!

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9 14. V the exemption of the noble gases, why is an element with a high ionization energy likely to have a high electron affinity? A: (p. 133, 134, 139) Atoms with high ionization energies are really attracted to your electrons. They want to keep them. That takes a lot of of energy to pull them away. Similarly, atoms v high electron affinity room attracted to electrons. They additionally want electrons. This is not true because that noble gases because noble gases just want to remain the way they are.

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Notes: To number this out, incorporate the reasoning behind ionization energy and also electron affinity.

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