Table of Contents
- 1 How does number of electrons affect atomic radius?
- 2 How does losing electrons affect atomic radii?
- 3 What are the factors that affect the atomic radius of an element?
- 4 Why does ionic radii increase down a group?
- 5 What affects ionic radii?
- 6 What is atomic radii and write the factor affecting on it?
- 7 How does atomic radii changes in a group and why?
- 8 Why does the atomic radii decrease as you move across the periodic table?
- 9 Why are electrons more easily removed from an atom?
How does number of electrons affect atomic radius?
As the atomic number of an element increases, so does the size of its nucleus and the number of electrons around it. The bigger the atomic number, the larger the atom’s radius. The growing size is due to the increasing number of filled electron shells as you move down the periodic table.
How does losing electrons affect atomic radii?
Neutral atoms tend to increase in size down a group and decrease across a period. When a neutral atom gains or loses an electron, creating an anion or cation, the atom’s radius increases or decreases, respectively.
What are the factors that affect the atomic radius of an element?
Explanation of the general trends
| factor | principle | effect on radius |
|---|---|---|
| nuclear charge | attractive force acting on electrons by protons in nucleus | decreases the atomic radius |
| shielding | repulsive force acting on outermost shell electrons by inner electrons | increases the atomic radius |
Why does the atomic radius decrease as electrons are added?
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. Since the force of attraction between nuclei and electrons increases, the size of the atoms decreases.
Does atomic radii increase with atomic number?
As the atomic number increases along each row of the periodic table, the additional electrons go into the same outermost shell, causing the atomic radius to decrease due to the increasing nuclear charge.
Why does ionic radii increase 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. Ionic radius is the distance from the nucleus to the outer edge of the electron cloud of an ion.
What affects ionic radii?
Ionic size (for the same ion) also increases with increasing coordination number, and an ion in a high-spin state will be larger than the same ion in a low-spin state. In general, ionic radius decreases with increasing positive charge and increases with increasing negative charge.
What is atomic radii and write the factor affecting on it?
Factors Affecting Atomic Size: Number of Shells: Atomic size increases with the increase in the number of electronic shells. Nuclear Charge: As the nuclear charge increases the atomic radius decreases due to increase in the attractive force on the outermost electrons.
How does the atomic radii will change as electrons are added to a shell?
The gain of an electron adds more electrons to the outermost shell which increases the radius because there are now more electrons further away from the nucleus and there are more electrons to pull towards the nucleus so the pull becomes slightly weaker than of the neutral atom and causes an increase in atomic radius.
Which of the following explains why the atomic radii decrease across a period?
As you move across the period, the number of protons increases, which increases the nuclear charge. The number of electrons remains the same creating a larger Coulombic attraction and decreasing the radii.
How does atomic radii changes in a group and why?
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.
Why does the atomic radii decrease as you move across the periodic table?
Atomic radii decrease, however, as one moves from left to right, across the Periodic Table. Although more electrons are being added to atoms, they are at similar distances to the nucleus; and the increasing nuclear charge “pulls” the electron clouds inwards, making the atomic radii smaller.
Why are electrons more easily removed from an atom?
The shielding effect explains why valence shell electrons are more easily removed from the atom. The nucleus can pull the valence shell in tighter when the attraction is strong and less tight when the attraction is weakened. The more shielding that occurs, the further the valence shell can spread out.
Why do atoms of Group 16 have lower ionization energies?
Atoms of Group 16 (O, S, etc.) have lower ionization energies than atoms of Group 15 (N, P, etc.). Hund’s rule is behind the explanation. In a nitrogen atom, there are three electrons in the 2 p sublevel and each is unpaired. In an oxygen atom, there are four electrons in the 2 p sublevel, so one orbital contains a pair of electrons.
How are atomic radii different for different types of atoms?
To a first approximation we can regard atoms as “hard spheres”, with an outer radius defined by the outer electron orbitals. However, even for atoms of the same type, atomic radii can differ, depending on the oxidation state, the type of bonding and – especially important in crystals – the local coordination environment.