Periodic properties

A group consist of?

Of elements in the same column

Elements in a group have the same number of?

Valence electrons, which are the electrons in outermost subshell

A period consists of?

Elements that occupy the same row

Elements in a period have the same number of?

electrons shells

The atomic number of an element is equal to the number of?

Protons

Group1 elements in a periodic table are called?

Alkali metals

Group 2 elements in the periodic table are called?

Alkaline earth metals

Group 3-12 elements in the periodic table are called?

Transition metals

Group 12-17 elements in the periodic table are called?

metalloids ( only some which are B,Si, Ge, As, Sb, Te, and Po)

Group 17 elements in the periodic table are called?

Halogens

Group 18 elements in the periodic table are called?

Noble gases

What is oxidation state?

The number of electrons that an atom loses, gains, or appears to use when bonding with another atom

What elements have multiple oxidation states?

Transition metals

In what row are transition metals colorless?

Row 4

What are the two inner transition metals?

Lanthanides and actinides

lanthanides are in what period?

Period 6

lanthanides are in what period?

Period 6

What is the most prominent oxidation state for transition metals is?

+2

What is the most prominent oxidation state for inner transition metals is?

+3

What are the diatomic atoms?

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, and Bromine

Malleable and lustrous is a characteristic of?

Metals

Good conductors of electricity/ heat are a characteristic of?

Metals

Form basic oxides are a characteristic of?

Metals

Lose electrons to form cations are a characteristic of?

metals

Usually solid at room temperature, with the exception of mercury (Hg), which is liquid are a characteristic of?

Metals

Generally, high melting and boiling points are a characteristic of?

Metals

Brittle, dull are a characteristic of?

Non-Metals

Poor conductors of electricity/ heat are a characteristic of?

Non-metals

Form acidic oxides are a characteristic of?

Non-metals

Gain electrons to form anions are a characteristic of?

Non-Metals

Gas or solid at room temperature, with the exception of bromine (Br), which is liquid are a characteristic of?

Non-Metals

Generally, low melting and boiling points are a characteristic of?

Non-metals

What is Atomic Radius?

Half the distance between the nuclei of two identical atoms bonded together

What is the trend of the atomic radius?

Atomic radius increases from right to left across a period and increases going down a group

What is the effect of the atomic radius increasing from right to left across a period?

The number of protons in an atom decreases from right to left. The decreasing number of protons results in a weaker nuclear attraction between the protons and electrons, which results in electron shells being further apart from the nucleus, therefore increasing the radius

What is the effect of the atomic radius increasing when going down a group?

The number of electron shells increases. Each additional electron level gets further and further away from the nucleus, which causes the atomic radius to increase

What is an effective nuclear charge?

Is the amount of positive charge experienced by an electron.

How is the effective nuclear charge calculated?

Zeff= Z-S

z= number of protons

s= number of shielding (non-valence electrons)

What is the trend of the effective nuclear charge?

Increase left to right across a period an increase going up a group

What is the effect of increasing the effective nuclear charge when going left to right across a period?

The number of protons increases without an increase in electron shells, and thus without an increase in the shielding effect. This results in electrons being pulled closer to the nucleus due to a stronger attraction.

What is the effect of the effective nuclear charge increasing when going up a group?

As the number of electron shells decreases, the outer-shell electrons move closer to the positively charged nucleus. This increase effective nuclear charge.

What is Isoelectronic series?

They are atoms that have an identical number of electrons but a different number of protons.

What are anions?

Are ions that have gained electrons and have more electrons than protons, making them negatively charged

What are cations?

Are ions that have lost electrons and have more protons than electrons, making them positively charged.

What is the radius of an anion? why?

It has a larger radius due to increased electron-electron repulsion. This expands the size of the electron cloud, resulting in a larger radius.

What is the radius of a cation? why?

It has a smaller radius due to the decrease in the number of electrons, which reduces electron-electron repulsion. This reduces the size of the electron cloud, resulting in a smaller radius

What is Ionization energy?

Energy needed to remove an electron from an atom

What is the trend in ionization energy?

Ionization energy increase going from left to right across a period and increase up a group

What is the effect of the Ionization energy increasing when going left to right across a period?

The atomic number, or the number of protons, increases. As the valence shell continues to fill, the electrons become harder to remove (require more energy) due to an increase in effective nuclear charge,

What is the effect of the Ionization energy increasing when going up a group?

There are fewer electron shells and, consequently, less of a shielding effect from the inner electrons. This creates difficulty in removing the electrons from the valence shells

What are the two notable exceptions of the Ionization energy? why?

1. Alkaline earth metals: have filled orbitals, which gives them greater stability, leading to their higher ionization energy compared to group 13 elements in the same period.

2. Group 15 elements: Have half-filled orbitals, which gives them greater stability, leading to their higher ionization energy compared to group 16 elements in the same period

What is electron affinity?

The amount of energy released when an electron is added to an atom

What is the trend for electron affinity?

Increase going from left to right across a period and increase going up a group

What is the effect of the electron affinity increasing when going left to right across a period?

As the atom’s valence shell gets filled, there is increased attraction between the nucleus and the electrons of the atom. This creates a stronger affinity for electrons

What is the effect of the electron affinity increasing when going up a group?

There are fewer electron shells, leading to decreased electron shielding and greater proximity between the nucleus and the valence electrons, thereby increasing nuclear attraction and thereby increasing electron affinity.

What are the three notable exceptions for electron affinity? why?

1. Group 2: have filled s-orbitals, so their electron affinities are very low

2. Group 15: have half-filled orbitals, p-orbitals, so their electron affinities are lower than those of the group 14 elements of the same period

3. Noble gases: Filled electron shells, so their electron affinities are negligible

What is electronegativity?

The measurement of an atom’s ability to attract electrons in a bond. The higher an atom's electronegativity, the greater its ability to attract electron pairs.

What is the trend of electronegativity?

Increase from left to right across a period and within a group.

What is the effect of the electronegativity increasing when going left to right across a period?

With increasing protons as you go from left to right across a period, the ability of an atom to attract an electron pair is increased.

What is the effect of the electronegativity increasing when going up a group?

As the atomic radius decreases, and the valence electrons experience less shielding, the ability of an atom to attract an electron pair is increased.