Questions and Answers
In what period is cesium, atomic number 55?
Period 6
The alkali metals belong to the _______-block in the periodic table.
s
Aluminum, atomic number 13, is in which period?
Period 3
What is the group name for the 14 elements in the sixth period that have occupied 4f orbitals?
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The electron configuration of an element is [Kr] 5s² 4d⁵. To what group does this element belong?
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Elements in which the d-sublevel is being filled have the properties of what?
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What sublevel(s) is (are) being filled in Period 3?
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To what group does magnesium, atomic number 12, belong?
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The elements whose electron configurations end with p⁵ in the highest occupied level belong to which group?
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To what group does nitrogen belong, with an electron configuration of 1s² 2s² 2p³?
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In what period is calcium, atomic number 20?
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The electron configurations of the noble gases from neon to radon in the periodic table end with filled what?
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Which orbitals are characteristic of the lanthanide elements?
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What is the group name for the soft, silvery active metals with one electron in an s orbital?
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To what group does strontium belong, with its highest occupied level at 5s²?
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To what group does titanium, atomic number 22, belong?
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Periods with elements filling f-sublevels are assigned group numbers.
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In Period 4, how many elements have electrons in the d sublevel?
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Study Notes
Electron Configurations and Periodic Table
- Cesium (atomic number 55) has the electron configuration [Xe] 6s¹, located in Period 6.
- Alkali metals occupy the s-block in the periodic table.
- Aluminum (atomic number 13) shows electron configuration [Ne] 3s² 3p¹, placing it in Period 3.
- The lanthanides consist of 14 elements in Period 6 that fill the 4f orbitals.
Group Identification
- An element with the configuration [Kr] 5s² 4d⁵ belongs to Group 7.
- D-sublevel filling transforms elements into metals.
- In Period 3, the filling sublevels are s and p.
- Magnesium (atomic number 12) has an electron configuration of [Ne] 3s², thus belongs to Group 2.
Noble Gases and Group Characteristics
- Elements with electron configurations ending in p⁵ are classified in Group 17.
- Nitrogen's electron configuration is 1s² 2s² 2p³, placing it in Group 15.
Period and Group Findings
- Calcium (atomic number 20) has an electron configuration [Ar] 4s², situating it in Period 4.
- Noble gases from neon to radon have electron configurations that end with filled p orbitals.
- Lanthanides are characterized by their f orbitals.
Properties of Various Groups
- Alkali metals are soft, silvery active metals with one electron in an s orbital.
- Strontium's highest occupied energy level is 5s², categorizing it in Group 2.
- Titanium (atomic number 22) with the configuration [Ar] 4s² 3d² is classified under Group 4.
Period Information
- Periods containing elements that fill f-sublevels are not assigned specific group numbers.
- In Period 4, 16 out of 18 elements possess electrons in the d sublevel.
Studying That Suits You
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Description
Test your understanding of electron configurations and periodic table placements with these flashcards based on Chemistry Chapter 6.2.2. Learn about alkali metals, periods, and specific elements like cesium and aluminum. Perfect for reinforcing your knowledge in chemistry topics related to the periodic table.
