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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.
Why does the general electronegativity trend increases across the same period?
The general electronegativity trend increases across the same period due to the increasing effective nuclear charge, which attracts the electrons more strongly towards the nucleus. As you move from left to right across a period, the number of protons in the nucleus increases while the shielding effect remains relatively constant, resulting in a greater attraction for electrons and higher electronegativity values.
What general statement can summarize the trend in the ionization energy when moving across a period of element?
The ionization energy generally increases across a period from left to right. This is because as you move across a period, the effective nuclear charge increases, making it more difficult to remove an electron. Additionally, the increasing number of protons in the nucleus leads to stronger attraction between the nucleus and the electrons.
What happened to atomic mass when across each period?
As you move across a period in the periodic table from left to right, the atomic mass generally increases. This is due to the addition of protons and neutrons in the nucleus, which contributes to a higher mass. However, this trend is not perfectly linear, as variations in isotopes and electron configurations can cause slight fluctuations in atomic mass values. Overall, the increase reflects the addition of heavier elements as you progress across the period.
What happens to the characteristics of atoms in a period as you go across a period?
As you move across a period in the periodic table, the atomic number increases, leading to a greater positive charge in the nucleus. This results in stronger attraction between the nucleus and the electrons, causing a decrease in atomic radius. Additionally, elements generally become less metallic and more non-metallic, with increasing electronegativity and ionization energy as you progress from left to right across the period.
Why do atoms get smaller across a period?
Atoms get smaller across a period because the increasing number of protons in the nucleus pulls the electrons closer to the nucleus, resulting in a stronger attraction and a smaller atomic size.
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.
Why does the general electronegativity trend increases across the same period?
The general electronegativity trend increases across the same period due to the increasing effective nuclear charge, which attracts the electrons more strongly towards the nucleus. As you move from left to right across a period, the number of protons in the nucleus increases while the shielding effect remains relatively constant, resulting in a greater attraction for electrons and higher electronegativity values.
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.
What is the most important in determining the periodic trends across a period?
The nuclear charge, or number of protons in the nucleus, is the most important factor in determining periodic trends across a period. As you move across a period, the nuclear charge increases, leading to stronger attraction between the nucleus and the electrons, affecting properties such as atomic size and ionization energy.
What is is the trend across a period?
The trend across a period refers to how a property of elements changes as you move from left to right across a row in the periodic table. For example, in terms of atomic size, the trend across a period is generally a decrease due to the increasing number of protons in the nucleus pulling the electrons closer.
What general statement can summarize the trend in the ionization energy when moving across a period of element?
The ionization energy generally increases across a period from left to right. This is because as you move across a period, the effective nuclear charge increases, making it more difficult to remove an electron. Additionally, the increasing number of protons in the nucleus leads to stronger attraction between the nucleus and the electrons.
What trend in ionization energy occurs going across a period on the periodic table and why?
Ionization energy generally increases across a period from left to right on the periodic table. This trend occurs because as you move across a period, the number of protons in the nucleus increases, resulting in a greater nuclear charge. This stronger attraction between the nucleus and the outer electrons requires more energy to remove an electron, thus increasing the ionization energy.
What happened to atomic mass when across each period?
As you move across a period in the periodic table from left to right, the atomic mass generally increases. This is due to the addition of protons and neutrons in the nucleus, which contributes to a higher mass. However, this trend is not perfectly linear, as variations in isotopes and electron configurations can cause slight fluctuations in atomic mass values. Overall, the increase reflects the addition of heavier elements as you progress across the period.
Why does the ionization energy increase across a period?
The ionization energy increases across a period because as you move from left to right, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons. This makes it harder to remove an electron, resulting in higher ionization energy.
What happens to the characteristics of atoms in a period as you go across a period?
As you move across a period in the periodic table, the atomic number increases, leading to a greater positive charge in the nucleus. This results in stronger attraction between the nucleus and the electrons, causing a decrease in atomic radius. Additionally, elements generally become less metallic and more non-metallic, with increasing electronegativity and ionization energy as you progress from left to right across the period.
What happens to the atomic radius as you go across a period?
It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
