What is the electron configuration the following?
3. Arsenic
4. Lead

3. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

4. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d10 4f14 6p2

Explanation:

Divide the periodic tables into blocks to find electron configurations.

Groups 1-2 are the s block.

Groups 13-18 are the p block.

Groups 3-12 are the d block (excluding Lanthanides and Actinides).

The Lanthanides and Actinides are the f block.

To find the electron configuration of arsenic, move across the periodic table starting from the top left corner of the periodic table. H and He (which is actually part of the s block) are 1s2 (period, followed by block, followed by how many elements over). Move to the next period (2). Li and Be are 2s1 and 2s2 respectively, but we would only write 2s2 in our configuration (the last/rightmost of the block). Then we have 2p6, which passes B, C, N, O, F, and Ne. We continue this process: 3s2, 3p6, and 4s2. Now we reach the d block (Groups 3-12). The period of these elements will be written 1 less (for example, Scandium would not be ...4d1; instead, it would be ...3d1). So we continue: 3d10, and then back onto the 4th period in the p block. Since arsenic is 3 elements over in the p block, we will finish the configuration with 4p3.

As for lead, you will have to pass the lanthanides, which are f block. They are similar to the d block, except you write the period as 2 less (for example, Cerium would be ...4f1, rather than 6f1). The elements lanthanum and actinium are not in the f block; they are in the d block.

One more thing to note are noble gas configurations. Noble gas configurations use the Group 18 gases (noble gases) to simplify our configurations. Let's take arsenic as an example again: since the noble gas before arsenic is argon, Ar (the element in group 18 in the previous period), we can write argon in brackets, [Ar], and then write only the configuration of the period arsenic is in: 4s2 3d10 4p3. As a result, our noble gas configuration for arsenic would look like this: [Ar] 4s2 3d10 4p3.

The noble gas configuration for lead is [Xe] 6s2 5d10 4f14 6p2.

Sorry for the long response, but I wanted to clarify the method to approach these types of problems for the future. I hope you at least get a general idea of how to solve these problems. :)

answer: your mm

explanation:

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.