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What is the relationship between the atomic number of an element and its effective nuclear charge, specifically in the case of oxygen?
The atomic number of an element is the number of protons in its nucleus, which determines its effective nuclear charge. In the case of oxygen, which has an atomic number of 8, the effective nuclear charge is the attraction felt by the outermost electrons towards the nucleus, and it increases as the atomic number increases.
What are the three concepts that can be used to explain the different periodic trends?
Atomic size: Refers to the distance between the nucleus and the outermost electrons. It decreases across a period due to increasing nuclear charge pulling electrons closer. Ionization energy: The energy required to remove an electron from an atom. It increases across a period due to stronger nuclear charge. Electronegativity: The ability of an atom to attract electrons in a chemical bond. It increases across a period due to stronger nuclear charge and smaller atomic size.
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 periodic trends are inversely proportional to effective nuclear charge?
Atomic radius and ionization energy are inversely proportional to effective nuclear charge. As the effective nuclear charge increases, the attraction between the nucleus and the electrons increases, causing the atomic radius to decrease. In contrast, the ionization energy increases because it becomes harder to remove an electron from the atom due to the stronger attraction.
What trend does electronegativity follow?
In electronegativity, the first ionization energy increases as it moves from left to right across a period . The nuclear charge also increases and the shielding effect is constant when moving across.
Nuclear charge increases across a period atoms become?
The atoms become smaller in atomic radius.
Does nuclear charge increases as you move from left to right across the periodic table?
moving from left to right across a period, one electron is added for each element.example: Boron has 3, Carbon has 4.
What happens when the nuclear charge increases across a period?
As the nuclear charge increases across a period, the number of protons in the nucleus increases. This leads to a stronger attraction between the nucleus and the electrons in the atom, resulting in a greater effective nuclear charge. This can lead to an increase in the atomic size and higher electronegativity across a period.
How does size change in a period and in a group?
Atomic size decreases across a period as the effective nuclear charge increases. Atomic size increases down a group as the energy level (shells) increases.
How does atomic radius vary in group and in period on periodic table?
Down a period the atomic radius increases as the number of shells (or energy levels) increases. Across a period the atomic radius decreases as the effective nuclear charge increases.
What to atomic properties have an increasing trend as you move across the periodic table?
As we move across a period, electronegativity increases. Ionization enthalpy also increases because of increasing nuclear charge.
What is the trend in atomic size across the period from sodium to argon?
Atomic size decreases across the period from sodium to argon due to increasing nuclear charge, which attracts the outermost electrons more strongly, pulling them closer to the nucleus. This results in a smaller atomic size as you move from left to right across the period.
What effect on atomic size is more significant an increase in nuclear charge across a period or an increase in occupied energy levels within a group?
An increase in nuclear charge across a period has a more significant effect on atomic size than an increase in occupied energy levels within a group. As the nuclear charge increases, the attraction between the positively charged nucleus and the negatively charged electrons strengthens, pulling the electrons closer and resulting in a decrease in atomic size. In contrast, while the addition of energy levels down a group increases atomic size due to greater electron shielding and distance from the nucleus, the effect of increased nuclear charge across a period is dominant in reducing atomic size.
What is the relationship between the atomic number of an element and its effective nuclear charge, specifically in the case of oxygen?
The atomic number of an element is the number of protons in its nucleus, which determines its effective nuclear charge. In the case of oxygen, which has an atomic number of 8, the effective nuclear charge is the attraction felt by the outermost electrons towards the nucleus, and it increases as the atomic number increases.
What are the three concepts that can be used to explain the different periodic trends?
Atomic size: Refers to the distance between the nucleus and the outermost electrons. It decreases across a period due to increasing nuclear charge pulling electrons closer. Ionization energy: The energy required to remove an electron from an atom. It increases across a period due to stronger nuclear charge. Electronegativity: The ability of an atom to attract electrons in a chemical bond. It increases across a period due to stronger nuclear charge and smaller atomic size.
How do atomic radii change from left to right across a horizontal row of the periodic table and what is the main reason?
Atomic radii decreases on moving from left to right as the effective nuclear charge increases.
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.
