Simple electronic structure 2 ( Form 2, Chemistry )

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Test knowledge on groups, periods and electron filling.

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Simple electronic structure 2 ( Form 2, Chemistry )


Simple electronic structure 2 ( Form 2, Chemistry )Online version Test knowledge on groups, periods and electron filling. by YAKILI LMS 1 The Aufbau principle states electrons fill the lowest energy orbitals first. Yes No 2 The Aufbau principle combined with Pauli exclusion explains the periodic trends. Yes No 3 The noble gas configuration for argon is 1s2 2s2 2p6 3s2 3p6. Yes No 4 Pnictogens include nitrogen, phosphorus, and arsenic. Yes No 5 The 4s orbital fills before the 3d in many first-row transition metals when following Aufbau. Yes No 6 Group I elements are alkali metals. Yes No 7 3p orbitals begin to fill after 3s is filled. Yes No 8 Electron configuration 1s2 2s2 2p6 corresponds to neon. Yes No 9 A 3d subshell can hold up to ten electrons. Yes No 10 Group IV elements include carbon, silicon, and germanium. Yes No 11 Magnesium (Mg) is in period 3 and group 2. Yes No 12 Hydrogen is commonly placed in Group I or Group 1, though it is unique. Yes No 13 Hund's rule states electrons fill degenerate orbitals singly before pairing. Yes No 14 Sodium loses one electron to achieve a noble gas configuration. Yes No 15 Group VIII elements are the noble gases. Yes No 16 The statement 1s2 2s2 2p4 describes oxygen’s ground-state configuration is true. Yes No 17 The first period contains only two elements: hydrogen and helium. Yes No 18 Zinc’s common ground-state electron configuration is [Ar] 3d10 4s2. Yes No 19 Copper’s common ground-state electron configuration is [Ar] 3d10 4s1. Yes No 20 3s is lower in energy than 2p in most cases for second-row elements. Yes No 21 Nitrogen has a 2p3 valence configuration in the ground state. Yes No 22 Electron configurations determine the position of an element in the periodic table. Yes No 23 Chalcogens typically gain or share two electrons in reactions. Yes No 24 Group V elements are the pnictogens. Yes No 25 Electron configuration of carbon is 1s2 2s2 2p2. Yes No 26 Group II elements are alkaline earth metals. Yes No 27 Group VII elements are the halogens. Yes No 28 Oxygen has six electrons in its outer shell (valence electrons). Yes No 29 The electron pair repulsion in p orbitals follows Hund’s rule for maximum multiplicity. Yes No 30 Orbitals can hold up to two electrons with opposite spins in the same orbital. Yes No 31 Halogens are highly reactive nonmetals. Yes No 32 The group number can help identify valence electrons in main-group elements. Yes No 33 A period is a horizontal row in the periodic table. Yes No 34 The lanthanide and actinide series are often shown separately in periodic tables. Yes No 35 Aluminium (Al) is in period 3 and group 13. Yes No 36 Groups 1, 2, and 13-18 are main-group elements. Yes No 37 The periodic table is organized to reflect electron configurations. Yes No 38 2p orbitals can hold a maximum of six electrons. Yes No 39 A filled 1s orbital can hold a maximum of two electrons with opposite spins. Yes No 40 Chalcogens include oxygen, sulfur, and selenium. Yes No 41 Group III elements are the boron group. Yes No 42 For potassium, the electron configuration ends with 4s1. Yes No 43 Period length corresponds to the number of electron shells. Yes No 44 A group is a vertical column in the periodic table. Yes No 45 Fluorine has the highest electronegativity among the halogens in period 2. Yes No 46 Configurations can be condensed using noble gas shorthand. Yes No 47 The noble gases have completely filled p orbitals in their valence shells. Yes No 48 The maximum electrons in a p orbital set is six. Yes No 49 Electron shells are numbered by principal quantum number n. Yes No 50 The last filled shell in neon is the second shell (2). Yes No

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Simple electronic structure 2 ( Form 2, Chemistry )Online version

by YAKILI LMS

The Aufbau principle states electrons fill the lowest energy orbitals first.

The Aufbau principle combined with Pauli exclusion explains the periodic trends.

The noble gas configuration for argon is 1s2 2s2 2p6 3s2 3p6.

Pnictogens include nitrogen, phosphorus, and arsenic.

The 4s orbital fills before the 3d in many first-row transition metals when following Aufbau.

Group I elements are alkali metals.

3p orbitals begin to fill after 3s is filled.

Electron configuration 1s2 2s2 2p6 corresponds to neon.

A 3d subshell can hold up to ten electrons.

Group IV elements include carbon, silicon, and germanium.

Magnesium (Mg) is in period 3 and group 2.

Hydrogen is commonly placed in Group I or Group 1, though it is unique.

Hund's rule states electrons fill degenerate orbitals singly before pairing.

Sodium loses one electron to achieve a noble gas configuration.

Group VIII elements are the noble gases.

The statement 1s2 2s2 2p4 describes oxygen’s ground-state configuration is true.

The first period contains only two elements: hydrogen and helium.

Zinc’s common ground-state electron configuration is [Ar] 3d10 4s2.

Copper’s common ground-state electron configuration is [Ar] 3d10 4s1.

3s is lower in energy than 2p in most cases for second-row elements.

Nitrogen has a 2p3 valence configuration in the ground state.

Electron configurations determine the position of an element in the periodic table.

Chalcogens typically gain or share two electrons in reactions.

Group V elements are the pnictogens.

Electron configuration of carbon is 1s2 2s2 2p2.

Group II elements are alkaline earth metals.

Group VII elements are the halogens.

Oxygen has six electrons in its outer shell (valence electrons).

The electron pair repulsion in p orbitals follows Hund’s rule for maximum multiplicity.

Orbitals can hold up to two electrons with opposite spins in the same orbital.

Halogens are highly reactive nonmetals.

The group number can help identify valence electrons in main-group elements.

A period is a horizontal row in the periodic table.

The lanthanide and actinide series are often shown separately in periodic tables.

Aluminium (Al) is in period 3 and group 13.

Groups 1, 2, and 13-18 are main-group elements.

The periodic table is organized to reflect electron configurations.

2p orbitals can hold a maximum of six electrons.

A filled 1s orbital can hold a maximum of two electrons with opposite spins.

Chalcogens include oxygen, sulfur, and selenium.

Group III elements are the boron group.

For potassium, the electron configuration ends with 4s1.

Period length corresponds to the number of electron shells.

A group is a vertical column in the periodic table.

Fluorine has the highest electronegativity among the halogens in period 2.

Configurations can be condensed using noble gas shorthand.

The noble gases have completely filled p orbitals in their valence shells.

The maximum electrons in a p orbital set is six.

Electron shells are numbered by principal quantum number n.

The last filled shell in neon is the second shell (2).