periodic trends (practice)

Number the elements sodium, magnesium, and potassium in the predicted order of ionic radius from the largest (1) to the smallest (3). sodium magnesium potassium

2 3 1

Number the elements sodium, magnesium, phosphorus, and chlorine in the predicted order ionization energies from the highest to the smallest. sodium magnesium phosphorus chlorine

4 3 2 1

What is the predicted order of first ionization energies from highest to lowest for beryllium, calcium, magnesium, and strontium? Be > Ca > Mg > Sr Be > Mg > Ca > Sr Ca > Sr > Be > Mg Sr > Ca > Mg > Be

Be> Mg > Ca > Sr

Use the periodic table to select the element from the drop-down menu that has the correct relative electronegativity. Mg > P > C < Br <

Ca As N Cl

What is the predicted order of first ionization energies from highest to lowest for aluminum, phosphorus, silicon, and sulfur? Al > P > Si > S Al > Si > P > S S > P > Si > Al P > S > Si > Al

P > S > Si > Al

What are the trends and exceptions to the trends in electron affinity? Check all that apply. The electron affinities of the elements in Group 17 are larger (more negative) than the elements in Group 1. Electron affinities increase (become more negative) down a group. Elements in Group 14 have larger (more negative) electron affinities than elements in Group 15. Elements in Group 2 have very large electron affinities.

The electron affinities of the elements in group 17 are larger (more negative) than the elements in group 1 elements in group 14 have larger (more negative) electron affinities than elements in group 15

Electronegativity across a period: decreases. increases. Electronegativity down a group: decreases. increases.

increases decreases

Use the periodic table to determine which elements are likely to have a larger atomic radius than silicon (Si). Check all that apply. aluminum (Al) carbon (C) sulfur (S) tin (Sn)

aluminum (Al) tin (Sn)

Consider the elements bromine and chlorine; which element has a larger ionic radius? chlorine bromine

bromine

Consider the elements bromine and chlorine; which element has a higher ionization energy? chlorine bromine

chlorine

show the correct relationship of the electron affinities of the elements bromine and chlorine. Chlorine's electron affinity value is more negative than the electron affinity value of bromine. Bromine's electron affinity value is more negative than the electron affinity value of chlorine. This information cannot be determined using the periodic table.

chlorines electron affinity value is more negative than the electron affinity value of bromine

Describe the trends in atomic radii by checking the correct box. Atomic radii from the left to right across a period tend to: increase. decrease. Atomic radii from the top to the bottom of a group tend to: increase. decrease.

decrease increase

What are the periodic trends of ionic radii? Check all that apply. Ionic radii tend to increase down a group. Ionic radii tend to decrease across a period. Anionic radii tend to increase across a period. Cationic radii tend to decrease across a period. Ionic radii increase when switching from cations to anions in a period.

ionic radii tend to increase down a group cationic radii tend to decrease across a period ionic radii increase when switching from cations to anions in a period

Why are the trends and exceptions to the trends in ionization energy observed? Check all that apply. Ionization energy tends to increase down a group because the electrons get farther away from the nucleus. Ionization energy tends to increase across a period because the nuclear charge increases. Ionization energy tends to increase across a period because electrons are added to the same main energy level. The ionization energies of the elements in Group 16 tend to be slightly smaller than the elements in Group 15 because the fourth electron is added to an unfilled p orbital. The ionization energies of elements in Group 13 tend to be lower than the elements in Group 2 because the full s orbital shields the electron in the p orbital from the nucleus.

ionization energy tends to increase across a period because the nuclear charge increases the ionization energies of the elements in group 16 tend to be slightly smaller than the elements in group 15 because the fourth electron is added to an unfilled p orbital the ionization energies of the elements in group 13 tend to be lower than the elements in group 2 because the full s orbital shields the electron in the p orbital from the nucleus

show the correct relationship of the electron affinities of the elements sodium and phosphorus. Sodium's electron affinity value is more negative than the electron affinity value of phosphorus. Phosphorus' electron affinity value is more negative than the electron affinity value of sodium. This information cannot be determined using the periodic table.

phosphorus electron affinity value is more negative than the electron affinity value of sodium

A sodium cation is ______ than a sodium atom. A phosphorus anion is ______ than a phosphorus atom. A magnesium ion is _____ than a sodium ion. A chlorine ion is _____ than a phosphorus ion. A potassium ion is _____ than a sodium ion.

smaller larger smaller smaller larger