Frequent question: Which element in Group 2 has the largest radius?

Which element has the largest radius?

Explanation: Francium has the largest, Helium has the lowest. Atomic radius increases as you go to the left and downward due to the attraction of electrons and the nucleus in an atom.

What is the trend in Group 2?

Group 2 Elements are called Alkali Earth Metals. They are called s-block elements because their highest energy electrons appear in the s subshell. Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element. Going down the group, the first ionisation energy decreases.

What is the trend in atomic radius across Period 2?

Atomic radius is the distance from the atom’s nucleus to the outer edge of the electron cloud. In general, atomic radius decreases across a period and increases down a group. Across a period, effective nuclear charge increases as electron shielding remains constant.

Which alkali metal has the largest atomic radius?

(A) Comparison of Atomic and Ionic Radius of Group 1 (IA, alkali metals) Elements

What element has the smallest 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.

Which has the largest 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.

Is Group 1 or Group 2 more reactive?

The outermost electrons of the alkaline earth metals (group 2) are more difficult to remove than the outer electron of the alkali metals, leading to the group 2 metals being less reactive than those in group 1.

Which element in Group 2 has the smallest atomic radius?

Trends in Atomic Radius of Group 2 Elements

What is the trend in boiling points in Group 7?

The melting points and boiling points of the halogens increase going down group 7. This is because, going down group 7: the molecules become larger. the intermolecular forces become stronger.

What is the trend for atomic radius?

Periodic Trend

The atomic radius of atoms generally decreases from left to right across a period. … Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge.

Does atomic radius increase with atomic number?

1 Answer. The atomic number is the amount of protons present in the atom. Because of that, we can say that the atomic number represents the positive charge of the atom. As the positive charge of the atom increases the atomic radius decreases because the positive charge will bring electrons closer to the nucleus.

How do you determine atomic radius?

Divide the distance between the nuclei of the atoms by two if the bond is covalent. For example, if you know the distance between the nuclei of two covalently bonded atoms is 100 picometers (pm), the radius of each individual atom is 50 pm.

Which alkali metal is the biggest?

• francium. The heaviest of the alkali metals is very rare and radioactive and has a very short life span (about 22 minutes).
• cesium. Rare metal that is used especially in photoelectric cells, atomic clocks, infrared lamps and treating certain cancers.
• rubidium. …
• potassium. …
• sodium. …
• lithium.

Which noble gas has the largest atomic radius?

As you go down a group, the atomic radius increases because you are adding energy levels that are farther away from the nucleus. Smallest to Largest: Helium.
…
Largest to Smallest:

• Helium (highest ionization level in the periodic table)
• Neon.
• Argon.
• Krypton.
• Xenon.
• Radon.

Are alkali metals soft or hard?

The alkali metals are solids at room temperature (except for hydrogen), but have fairly low melting points: lithium melts at 181ºC, sodium at 98ºC, potassium at 63ºC, rubidium at 39ºC, and cesium at 28ºC. They are also relatively soft metals: sodium and potassium can be cut with a butter knife.