Explanation:

The group number is the very same as the number of the valence electron each facet within that team has. Therefore, two facets in the same team will have the same number of valence electrons. Since all bonding and/or ionizations involve the valence covering of electrons, atoms v the same variety of valence electron behave similarly. Both tellurium and sulfur are in group VI, and also have 6 valence electrons.

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Explanation:

The period number/row number is the energy level because that each element. Therefore, 2 atoms found in the very same row top top the periodic table have the same power level. Potassium and selenium are both in row 4 that the periodic table. Their highest energy level for electrons is 4.

Explanation:

Ionization power is the energy required to remove an electron. Noble gases room special since the have a complete valence covering of electrons, which renders them the many stable elements, and to remove an electron requires a many energy. The tendency for ionization energy is together follows: ionization energy increases native left to best within a row and from bottom to peak within a group on the regular table. All of the answer options are in the very same row of the routine table, however fluorine is the furthest come the right. Thus fluorine has the biggest ionization energy.

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### Example inquiry #14 : The routine Table

How countless valence electrons does the element oxygen have?

Explanation:

For neutral atoms, the number of valence electrons is same to the atom"s main group number. Follow to the periodic table, oxygen is in group 6; therefore, it has actually 6 valence electrons in its external shell.

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### Example inquiry #15 : The periodic Table

Which that the adhering to is the most electronegative element?

Fluorine

Oxygen

Chlorine

None that the answer selections are correct

Nitrogen

Fluorine

Explanation:

Generally speaking, as you go across a period and increase a team on the routine table, electronegativity increases. Fluorine is the most electronegative element, through a Pauling range electronegativity ranking of approximately 4.0.

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### Example inquiry #16 : The routine Table

Which that these facets is the very least likely to host on come its valence electrons once in the existence of a highly electronegative atom?

Iron

Sodium

Cobalt

Cesium

Rubidium

Cesium

Explanation:

Atomic radii increases from right to left of the routine table and it decreases bottom to top. Therefore francium, in the bottom left of the routine table, has the biggest atomic radius; helium, in the height right the the chart, has actually the smallest atomic radius. Based upon these trends, cesium would be the very least likely to hold on to its valence electrons due to the fact that it has actually a larger atomic radius compared to cobalt or iron. To compare this to helium which has actually a little atomic radius and a complete valence covering of electrons, which provides it really stable.

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### Example question #17 : The regular Table

Which the the complying with groups of elements would require the greatest influx of energy to dislodge one electron native its valence shell?

Transition metals

Alkaline earth metals

Alkali metals

Nonmetals

Halogens

Halogens

Explanation:

Halogens would need the greatest very first ionization energy to dislodge one of their valence shell electrons since they have both the biggest electron affinity and the smallest atomic radii. Since their electrons room both closer to your nuclei and halogens are much more "electron greedy" (electronegative), they require an ext energy to remove an electron. However, because the noble gasses have full valence shells, they have the greatest an initial ionization energies.

See more: How Long Is 58 Cm In Inches In 58 Cm? 58 Cm To Inches

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### Example inquiry #18 : The routine Table

You space tasked v packing a very small jar through as countless individual atom of the same facet as possible. Which element would you choose to ensure the biggest quantity of atoms would certainly fit in to the jar?

Francium

Boron

Helium

Hydrogen

Helium

Explanation:

Atomic radii decrease from left come right across the routine table and increase from height to bottom of the periodic table. Based upon these trends, helium has the smallest atomic radii and much more atoms would fit within our imaginary container.

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### Example question #19 : The regular Table

Which that these elements is most most likely to kind a polar bond?

Oxygen

Chlorine

Bromine

Fluorine

Nitrogen

Fluorine

Explanation:

Electronegativity is the propensity of one atom to lure electrons come it. Electronegative atoms room electron "greedy". When they form covalent bonds, highly electronegative atoms often form polar covalent binding in which the electrons spend a better amount of time near the electronegative atom resulting in a dipole moment. Water is the quintessential example of a polar molecule.

Electronegativity increases from left to right throughout the periodic table and increases native bottom to top as well. Fluorine is the many electronegative atom and also it would be most likely to an outcome in a polar molecule. Store in mind the the development of a polar bond relies on the differing electronegativities of the atom in question. Because that example, 2 oxygen atoms carry out not do a polar bond even though both atoms are extremely electronegative.

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### Example question #20 : The regular Table

Which the the following lists atom radius increasing from smallest to biggest?

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