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What happened to the atomis nucleus as you move across the period?
Wiki User
∙ 12y ago
it gets larger due to the addition of a proton and possibly neutrons.
Wiki User
∙ 12y ago
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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 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.
Why does the element with lowest atomic number have the greatest atomic radii in each period?
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
How does ionization enthalpy vary as you move across the periods vary from left to right?
in a period size decreases from left to right and hence electrons are more tightly held to the nucleus. so electron gain enthalpy increases across a period . down the period size increases and thus in general electron gain enthalpy decreses .
Why does the ionization energy decrease in a column?
Ionisation energy increases across a period and decreases down a group. This could be explained on the basis of their nuclear charge and atomic radii. As you move across a period, the nuclear charge goes on increasing and it becomes increasingly difficult to remove the outermost electron. As you move across a period, the atomic radii goes on decreasing. This implies that the valence electrons are strongly attracted by the nucleus. Hence it becomes difficult to remove the outermost loosely bound valence electron. Therefore, inonisation energy increases as we move across a period.
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 electrostatic interaction between the outermost electron and nucleus vary across the periodic table?
Across teh period, the atomic number increases and subsequently the number of protons in the nucleus increases. hence the extent of electrostatic attraction also varies.
Is a chlorine atom larger than a bromine?
Chlorine is in 3rd period and 17th group bromine is in 4th period and 17th group. The number of shells present in an atom is equal to the period no. In which it is present. So, chlorine has 3 shells while bromine has 4 shells. And atomis size is the distance between centre of nucleus and outermost shell. So, bromine atom is larger than bromine atom..
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.
What ahppens to the attraction between the nucleus and an electron when you move across a period?
As you move from left to right across a period, the attraction an atomic nucleus has for the atom's electrons increases. This is because positively charged, relatively heavy protons are being added to the nuclei as you move from left to right, and the additional protons have an increased attraction for the negatively charged and nearly weightless electrons.
Why does the element with lowest atomic number have the greatest atomic radii in each period?
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
Why nuclear charge increases when atomic number increases across a period?
Atomic number is the number of protons in the nucleus. The higher the number the higher the nuclear charge
What trends is there when you move form left to right across the second period of the periodic table?
When you move left to right across a period (for any period on the Table) the atomic radius decreases. For each atom as you progress to the right, an electron is added to the Principle Energy Level and a proton is added to the nucleus. Why is this important? Because the more positively-charged nucleus pulls the valence electron(s) in tighter. (When the electrons are pulled in closer to the nucleus, the size of the atom decreases.)
What element deviates from the trend in ionisation energy across period 2?
boron electros removed from 2p orbitals more shielded from the + nucleus so easily lost
Why do the properties of elements change across the period?
They change because the atomic number and mass differ from each other element. Going across the Periodic Table to the right, the atoms get smaller because another proton is added each time so the effective nuclear charge experienced by the electrons is greater and the electrons are pulled closer to the nucleus. Electronegativity increases as you progress across a period because smaller atoms are usually more likely to gain an electron. Ionization energy increases across a period because the atoms are smaller, pulled closer to the nucleus, so it takes more energy to break an electron away.
What is is the trend across a period?
what is the reason for ionization energy across a period
What factors need to be considered when predicting the trend in ionisation energies across a period?
The charge on the nucleus.The distance of the electron from the nucleus.The number of electrons between the outer electrons and the nucleus.
