What happens to electrons as you move from left to right?

What happens to electrons as you move from left to right?

Explanation: As you move from left to right, the nucleus gains protons. This increases the positive charge of the nucleus and its attractive force on the electrons. As a result, the valence electrons are held closer to the nucleus, and the atomic radius decreases.

How do trends change in the periodic table?

Periodic trends arise from the changes in the atomic structure of the chemical elements within their respective periods (horizontal rows) and groups in the periodic table. These laws enable the chemical elements to be organized in the periodic table based on their atomic structures and properties.

What happens to the number of electrons as you move from left to right on the table?

As the atomic number increases along a row of the periodic table, additional electrons are added to the same, outermost shell. The radius of this shell gradually contracts as the attraction between the additional electrons and the nucleus increases.

What is the trend of the periodic table when you move from left to right?

As you move left to right, the atomic radius gets SMALLER, so atoms hold on to their electrons more tightly and are more reactive. As you move down a group, the atomic radius gets LARGER, so atoms have a weaker hold on their electrons and are less reactive.

What is the trend in atomic radii as you move from left to right across a period?

Periodic Trend The atomic radius of atoms generally decreases from left to right across a period. There are some small exceptions, such as the oxygen radius being slightly greater than the nitrogen radius. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level.

Are there any exceptions to the atomic radius trend?

Periodic Trend The atomic radius of atoms generally decreases from left to right across a period. There are some small exceptions, such as the oxygen radius being slightly greater than the nitrogen radius. Since the force of attraction between nuclei and electrons increases, the size of the atoms decreases.

Why do both atomic size and ionic size increase as you move down a group?

As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period. While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms.

What is the trend in radii across a period?

In general, atomic radius decreases across a period and increases down a group. Across a period, effective nuclear charge increases as electron shielding remains constant.

What is the trend in atomic radii as you move from left to right across a period quizlet?

Atoms increase in size. Explain why Ionization energy increases/decreases as you move up/down and group and left to right across a period. Therefore, moving left to right across a period the nucleus has a greater pull on the outer electrons and the atomic radii decreases.

How does the tendency to gain electrons change on moving from left to right?

The tendency to gain electron increases as we go from left to right in a period because the effective nuclear charge increases and the atomic radius decreases. So the protons hold the electrons more tightly thus the loss of electrons become difficult.

How does the number of valence electrons change from left?

The number of valence electrons goes up by one each time you move another column (group) to the right. There are a few things to look out though when trying to figure out the number of valence electrons. Group 1 elements have one valence electrons, and Group 2 elements have 2 valence electrons.

Why do elements in the same period have the same number of electrons?

Elements in the same period have the same number of electron shells; moving across a period (so progressing from group to group), elements gain electrons and protons and become less metallic. This arrangement reflects the periodic recurrence of similar properties as the atomic number increases.

Why does electron affinity decrease from left to right?

Therefore, electron affinity decreases. Moving from left to right across a period, atoms become smaller as the forces of attraction become stronger. This causes the electron to move closer to the nucleus, thus increasing the electron affinity from left to right across a period. Electron affinity increases from left to right within a period.