Question

Indicate whether the following properties increase or decrease from left to right across the periodic table
a. atomic radius
b. first ionization energy
c. electronegativity (excluding noble gases)​

Answer 1

Answer: Here u go!

Explanation:

a) Atomic radius (excluding noble gases)  (Decrease)

b) First ionization energy  (Increase )

c) Electronegativity  ( Increase)

Hope this helps!(it took me a while sry)

Answer 2

The atomic radius will decrease, first ionization energy will increase, and electronegativity will increase from left to right across the periodic table.

Explanation:

• The horizontal rows in the periodic table are periods.
• When we move from left to right in the period the number of electrons and effective nuclear charge increases due to which the following properties increases:

1. Electronegativity is an ability of an atom to attract shared pair of electrons towards itself
2. First ionization enthalpy is an amount of energy required to remove an outermost electron from an isolated gaseous atom in its ground state.
3. Electron affinity is an amount of energy released when an electron is added to a neutral atom or molecule to form a negative ion.

• The atomic radius of the elements decreases on moving left to right in a period due to high nuclear charge electrons is highly attracted towards the nucleus.

So, from this, we can conclude that atomic radius will decrease, first ionization energy will increase, and electronegativity will increase from left to right across the periodic table.

Learn more about the periodic table here;

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