Question

what do you notice about the connection between the number of orbitals and the number of electrons the shell can hold? why is helium considered part of the s block? which two families of the periodic table make up the s block? which block are the noble gases & halogens in? which family makes up the d - block of the table? write down the correct aufbau order of shells below: when writing electron configurations, you always start with and work your way over from to until you get to. how does the order of writing electron configurations connect to the order of atomic numbers?

Explanation:

1. Each orbital can hold a maximum of 2 electrons. So the number of electrons a shell can hold is related to the number of orbitals in that shell. For example, the s - subshell has 1 orbital and can hold 2 electrons, the p - subshell has 3 orbitals and can hold 6 electrons.
2. Helium has its outermost electrons in the 1s orbital, so it is part of the s - block.
3. The alkali metals and alkaline - earth metals make up the s - block.
4. Noble Gases and Halogens are in the p - block.
5. The transition metals make up the d - block.
6. The Aufbau order of shells is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.
7. When writing electron configurations, you start with the lowest - energy shell (1s) and work your way over from the s - subshell to the p - subshell to the d - subshell to the f - subshell until you get to the appropriate number of electrons for the element.
8. The order of writing electron configurations follows the increasing order of energy levels. Atomic numbers increase as more electrons are added following the Aufbau principle, so the order of electron configurations is related to the order of atomic numbers as electrons are added to shells and subshells in a specific energy - based order.

Answer:

1. Each orbital can hold 2 electrons, so the number of electrons a shell can hold is 2 times the number of orbitals in that shell.
2. Helium has its outermost electrons in the 1s orbital.
3. Alkali metals and alkaline - earth metals.
4. p - block.
5. Transition metals.
6. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.
7. Lowest - energy shell (1s); s - subshell; p - subshell; d - subshell; f - subshell; appropriate number of electrons for the element.
8. The order of electron configurations follows the increasing order of energy levels which is related to the order in which atomic numbers increase as electrons are added following the Aufbau principle.