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An increase in the atomic number the atomic radius moving from left to right across a period.?
decreases
Atomic size generally as you go down a group?
Atomic size generally increases as you go down a group
Does elements on the periodic table decrease in atomic size when you move across a period from left to right and when you move down a group?
Atomic size generally decreases as you move across a period from left to right due to increasing effective nuclear charge. However, atomic size tends to increase as you move down a group due to the addition of more electron shells.
How does electronegativity change across the period?
Electronegativity tends to increase across a period from left to right. This is because as you move across a period, the nuclear charge increases and the atomic radius decreases, leading to a stronger attraction for electrons by the nucleus.
Does atomic density increase or decrease as we go across in a period?
It decreases across a period. Since the atomic number increases, so does no. of protons and electrons. This makes the electrostatic force of attraction between electrons larger and hence the atom shrinks a bit. This makes the radius smaller.
Why does atomic size increase from left to right across a period?
atomic size decreases across a period
An increase in the atomic number the atomic radius moving from left to right across a period.?
decreases
What does atomic radius do across a period?
Atomic radius tends to decrease across a period from left to right. This is because as you move across a period, the number of protons in the nucleus increases, leading to an increase in the effective nuclear charge felt by the outermost electrons, which pulls them closer to the nucleus.
Atomic size generally as you go down a group?
Atomic size generally increases as you go down a group
Ionization energies tend to do what from left to right across a period?
increase from left to right across a period.
Does elements on the periodic table decrease in atomic size when you move across a period from left to right and when you move down a group?
Atomic size generally decreases as you move across a period from left to right due to increasing effective nuclear charge. However, atomic size tends to increase as you move down a group due to the addition of more electron shells.
How do atomic numbers and atomic masses increase in the periodic table?
Atomic numbers increase from left to right across a period on the periodic table. This is because each element in a period has one more proton in its nucleus compared to the element before it. Atomic masses generally increase from left to right as well, but there may be deviations due to isotopes or other factors. Within a group or column, atomic numbers and atomic masses increase from top to bottom as each successive element has more electrons and neutrons than the one above it.
How does the atomic number change in a period?
When going left to right across a period, the atomic number of element increases.
Does an element on the periodic table decrease in atomic size when you move across a period from left to right and when you move down a group?
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
What is the pattern of atomic mass as you go across a period?
As you move across a period in the periodic table from left to right, the atomic mass generally increases. This increase is due to the addition of protons and neutrons in the nucleus of the atoms, which raises the overall mass. However, the increase is not perfectly linear, as isotopes and variations in neutron numbers can cause slight fluctuations in atomic mass values.
How does the atomic radius vary in a period?
Atomic radius decreases across a period from left to right, except for the noble gases.
How does electronegativity change across the period?
Electronegativity tends to increase across a period from left to right. This is because as you move across a period, the nuclear charge increases and the atomic radius decreases, leading to a stronger attraction for electrons by the nucleus.
