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- 1. Multiple ChoiceAs you move down the periodic table atoms get bigger. This is because ____________.The atoms have more mass.The atoms have more protons.The atoms have more energy levelsThe atoms have more neutrons
- 2. Multiple ChoiceAs you move across the periodic table atoms tend to get smaller because, ______________.the atoms have more mass.the atoms have less massthe atoms have greater core charge.the atoms have less core charge.
- 3. Multiple ChoiceThe electronegativity of chlorine is the highest in period three. Why?Chlorine has the GREATEST effective nuclear charge and an INcomplete valence level.Chlorine has the GREATEST effective nuclear charge and a complete valence level.Chlorine has the LOWEST effective nuclear charge and an INcomplete valence level.Chlorine has the LOWEST effective nuclear charge and an complete valence level.
- 4. Multiple ChoiceWhich periodic group has the smallest atomic radius?Alkali metalsHalogensNoble GasesTransition metals
- 5. Multiple Choice
Based on electronegativity trends in the periodic table, which of the following is the most likely value for the electronegativity of silicon?2.441.232.222.03 - 6. Multiple ChoiceAtomic radius generally increases as we move __________.down a group and from right to left across a periodup a group and from left to right across a perioddown a group and from left to right across a periodup a group and from right to left across a period
- 7. Multiple ChoiceIf an atom has 3 valence electrons, what charge will it have as an ion?+3-3+5-5
- 8. Multiple ChoiceIf an element gains 2 electrons, what charge will it have when it becomes an ion?+2-2-6-6
- 9. Multiple ChoicePut these in increasing of electronegativity order:
F, N, BB < N < FB < F < NN < F < BF < N < B - 10. Multiple ChoiceWhen a barium atom loses two electrons to forma Ba2+ ion, the electrons are lost from the ___________.5s orbital.5p orbital.4f orbital.6s orbital
- 11. Multiple ChoiceWhich has the greater effective nuclear force:
Cl or Al? Why?Cl;
Greater number of protons.Al;
Greater number of protons.Cl;
Greater number of main energy levels.Al;
Greater number of main energy levels. - 12. Multiple ChoiceThe successive ionization energies are most likely representative of which 4th period element?potassiumcalciumgalliumgermanium
- 13. Multiple ChoiceThe electron configurations below represent neutral atoms in the ground state. Which configuration represents the element with the highest 1st ionization energy?1s22s22p61s22s11s22s22p63s11s22s22p63s23p6
- 14. Multiple ChoiceThe graph shows that that ionization energy generally increases from left to right across a period due to the increase in effective core charge. HOWEVER, there are two exceptions to this trend. Why does IE decrease from Group 2 to Group 3?A drop in IE occurs between Groups 2 and 3 because the p electrons do not penetrate the nuclear region as greatly as s electrons do and are therefore not as tightly held.A drop in IE occurs between Groups 2 and 3 because the increased repulsion created by the first pairing of electrons in the p-orbitals outweighs the increase in Zeff and thus less energy is required to remove the electron.A drop in IE occurs between Groups 2 and 3 because there is an increase in Zeff while the number of main energy levels remains the same.A drop in IE occurs between Groups 2 and 3 because there is a decrease in Zeff while the number of main energy levels increases.
- 15. Multiple ChoiceThe graph shows that that ionization energy generally increases from left to right across a period due to the increase in effective core charge. HOWEVER, there are two exceptions to this trend. Why does IE decrease from Group 5 to Group 6?A drop in IE occurs between Groups 5 and 6 because the p electrons do not penetrate the nuclear region as greatly as s electrons do and are therefore not as tightly held.A drop in IE occurs between Groups 5 and 6 because the increased repulsion created by the first pairing of electrons in the p-orbitals outweighs the increase in Zeff and thus less energy is required to remove the electron.A drop in IE occurs between Groups 5 and 6 because there is an increase in Zeff while the number of main energy levels remains the same.A drop in IE occurs between Groups 5 and 6 because there is a decrease in Zeff while the number of main energy levels increases.
- 16. Multiple ChoiceHow does the radius of Ca2+ compare to the radius of a neutral atom of Ca? Why?Ca2+ radius is LARGER; Ca2+ has FOUR main energy levels, Ca also has FOUR.Ca2+ radius is SMALLER; Ca2+ has FOUR main energy levels, Ca also has FOUR.Ca2+ radius is LARGER; Ca2+ has THREE main energy levels, Ca has FOUR.Ca2+ radius is SMALLER; Ca2+ has THREE main energy levels, Ca has FOUR.
- 17. Multiple ChoiceHow does the radius of O2- compare to the radius of a neutral atom of O? Why?O2- radius is LARGER; O2- has GREATER e- to p+ ratio and increased e-/e- REPULSION.O2- radius is SMALLER; O2- has GREATER e- to p+ ratio and increased e-/e- REPULSION.O2- radius is LARGER; O2- has SMALLER e- to p+ ratio and increased e-/e- REPULSION.O2- radius is SMALLER; O2- has SMALLER e- to p+ ratio and increased e-/e- REPULSION.
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