[PDF] Mastering Periodic Trends PDF

[PDF] Mastering Periodic Trends

Atomic radius is the distance from the atom's nucleus to the outer edge of the electron cloud In general, atomic radius decreases across a period and increases

[PDF] 65 Periodic Variations in Element Properties

Describe and explain the observed trends in atomic size, ionization energy, The trends for the entire periodic table can be seen in Figure 6 31

[PDF] PERIODIC TRENDS The periodic table is arranged in order of

These periodic trends can clearly be seen in atomic radii, ionic radii, ionization energies and electronegativities These specific trends will be investigated

[PDF] ATOMIC SIZE

In this periodic table, the relative sizes (not absolute - there are no measurements) are shown The sizes of the noble gas atoms (gray) can't really be

[PDF] Element Entry Identification What is the Atomic Number? Terms

Check the Periodic Table to find out how many electrons each element actually has The atomic radius is a measure of the size of an atom The larger the

[PDF] The Periodic Table and Periodic Trends - SU LMS

These radii are generally not the same (part (d) in Figure 7 5 "Definitions of the Atomic Radius") Periodic Trends in Atomic Radii Because it is impossible

[PDF] Unit 32: The Periodic Table and Periodic Trends Notes

To find atomic radius, atoms are assumed to be spheres The electron cloud size determines the atomic radius for an atom The radius values are only estimates

[PDF] Can the properties of an element be predicted using a periodic table?

tions about atomic size, electronegativity, ionization energies, bonding, solubility, and reactivity In this activity you will look at a few periodic

[PDF] Mastering Periodic Trends

causing the electron cloud to expand (justifies trends across a period) 1 Atomic In general, atomic radius decreases across a period and increases down a group Electronegativity is the measure of the ability of an atom in a bond to attract

[PDF] 65 Periodic Variations in Element Properties

The trends for the entire periodic table can be seen in Figure 6 31 Covalent Radii of the Halogen Group Elements Atom Covalent radius (pm) Nuclear charge

[PDF] Unit 32: The Periodic Table and Periodic Trends Notes - LCWU

the elements in vertical columns by their atomic mass and found he could get horizontal groups of 3 or 4 that had similar The periodic table provides a map for all the elements: To find atomic radius, atoms are assumed to be spheres

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MASTERINGPeriodic Trends

Perfect your performance with periodicity!

Important Trend Terms

E?ective nuclear charge:

the net positive charge from the nucleus that an electron can "feel" attractions from. The core electrons are said to shield the

valence electrons from the full attractive forces of the protons in the nucleus. Shielding: core (nonvalence) electrons shield the valence electrons

from the full attractive forces of the protons in the nucleus. Electron-electron repulsions: due to their like charges, electron pairs orient themselves as far away as possible from each other, causing the electron cloud to expand (justifies trends across a period).

1. Atomic Radius

Atomic radius increases

Atomic radius is the

distance from the atom's nucleus to the outer edge of the electron cloud. In general, atomic radius decreases across a period and increases down a group. Across a period, e?ective nuclear charge increases as electron shielding remains constant. A higher e?ective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

2. Ionic Radius

MetalsNonmetals

Ionic radius increases

Ionic radius is the

distance from the nucleus to the outer edge of the electron cloud of an ion. The same trend of atomic radius applies once you divide the table into metal and nonmetal sections. A cation has a smaller radius than its neutral atom because it loses valence electrons. The "new" valence shell is held closer to the nucleus, resulting in a smaller radius for the cation. An anion has a larger radius than the neutral atom because it gains valence electrons. There are added electron/electron repulsions in the valence shell that expand the size of the electron cloud, which results in a larger radius for the anion.

3.Io nization EnergyIE increases

IE increases

Ionization energy (IE) is the energy required to remove the highest-energy electron from a neutral atom. In general, ionization energy increases across a period and decreases down a group. Across a period, e?ective nuclear charge increases as electron shielding remains constant. This pulls the electron cloud closer to the nucleus, strengthening the nuclear attraction to the outer-most electron, and is more di?cult to remove (requires more energy). Down a group, the number of energy levels (n) increase and the distance is greater between the nucleus and highest-energy electron. The increased distance weakens the nuclear attraction to the outer-most electron, and is easier to remove (requires less energy).

4.Electronegativity

Electronegativity increases

Electronegativity

increases Electronegativity is the measure of the ability of an atom in a bond to attract electrons to itself. Electronegativity increases across a period and decreases down a group. Towards the left of the table, valence shells are less than half full, so these atoms (metals) tend to lose electrons and have low electronegativity. Towards the right of the table, valence shells are more than half full, so these atoms (nonmetals) tend to gain electrons and have high electronegativity. Down a group, the number of energy levels (n) increases, and so does the distance between the nucleus and the outermost orbital. The increased distance and the increased shielding weaken the nuclear attraction, and so an atom can't attract electrons as strongly. Fluorine is the most electronegative element, whereas francium is the least electronegative element.

[PDF] Mastering Periodic Trends

MASTERINGPeriodic Trends

Perfect your performance with periodicity!

Important Trend Terms

E?ective nuclear charge:

1. Atomic Radius

Atomic radius increases

Atomic radius increases

Atomic radius is the

2. Ionic Radius

MetalsNonmetals

Ionic radius increases

Ionic radius increases

Ionic radius is the

3.Io nization EnergyIE increases

IE increases

4.Electronegativity

Electronegativity increases

Electronegativity

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