What element in the second period has the largest atomic radius group of answer choices?

The element in the second period that has the largest atomic radius is the Lithium (Li).

Which one of the elements from Group 2 has the largest atomic radii?

Trends in Atomic Radius of Group 2 Elements

Which element has the largest atomic radius?

Atomic radii vary in a predictable way across the periodic table. As can be seen in the figures below, the atomic radius increases from top to bottom in a group, and decreases from left to right across a period. Thus, helium is the smallest element, and francium is the largest.

What element in the second period has the largest atomic radius group of answer choices carbon lithium potassium neon?

The correct option is D. The elements in the second period are lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon. In the second period, the atomic radius of the elements decreases across the period, thus lithium has the highest atomic radius of 152 picometer while neon has the least [67 picometer].

Which of the following element of second period has second highest radius?

Properties of Elements in Period 2 of the Periodic Table

Which metal has the smallest atomic radius?

Helium has the smallest atomic radius. This is due to trends in the periodic table, and the effective nuclear charge that holds the valence electrons close to the nucleus. Atomic radius decreases as you move across a period from left to right and decreases as you move up a group from bottom to top.

Does atomic radius increase down Group 2?

Going down group 2: there are more filled shells between the nucleus and the outer electrons … … so the electrons in the higher energy levels are further from the nucleus … the atomic radius increases.

Which is larger k or k+?

These are electrons with “highest energy level”. When at neutral, the potassium ion in the form of K has an electronic configuration of: … The K+ ion has its outermost electrons on the third energy level now and is size is smaller than that of K ion. Hence, K is larger than K+.

Which has the largest atomic radius mg Si S or Na?

Therefore the largest atoms are on the left and the smallest on the right. So sodium (Na) has the largest atomic radius, as the valence electrons are the least attracted to the nucleus.

Which element has the largest atomic radius K or Na?

As an example, potassium (K) has a larger average atomic radius (220 pm)than sodium (Na) does (180 pm). The potassium atom has an extra electron shell compared to the sodium atom, which means its valence electrons are further from the nucleus, giving potassium a larger atomic radius.

What element in Period 2 has the most mass?

The element neon, in period 2, has the most mass.

What is the atomic radius of RB?

290 pm

Why does atomic radius increase down a group?

In general, atomic radius decreases across a period and increases down a group. … Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

Which element has lowest electronegativity value?

The element with the lowest electronegativity value is francium, which has an electronegativity of 0.7. This value uses the Pauling scale to measure electronegativity. The Allen scale assigns the lowest electronegativity to cesium, with a value of 0.659.

How does atomic radius change from left to right?

Atomic radius decreases from left to right within a period. This is caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius. … This is caused by electron shielding.

Who attempted to organize the elements into a table by increasing atomic mass?

The English chemist John Newlands (1838–1898), hypothesizing that the chemistry of the elements might be related to their masses, arranged the known elements in order of increasing atomic mass and discovered that every seventh element had similar properties (Figure 3.4. 1 ).