'Ionization energy decreases' diaporamas de présentation

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION. PHYSICAL SETTING CHEMISTRY. Jan 2015. Table. 1 According to the modern model of the atom, the nucleus of an atom is surrounded by one or more. electrons neutrons positrons protons. Table.

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Trends in the Periodic Table

Trends in the Periodic Table. The properties of the elements exhibit trends. These trends can be predicted using the periodic table and can be explained and understood by analyzing the electron configurations of the elements.

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Bond. Chemical Bond.

Bond. Chemical Bond. ELECTRONEGATIVITY The tendency of an atom to attract electrons to itself when it is bonded to another atom. Check out Figure 5-20 on page 151. Where are electronegativities the greatest? The least?. OCTET. The eight outer electrons in an atom. FACT:

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Ch. 6 Chemical Periodicity

Ch. 6 Chemical Periodicity. effective nuclear charge.

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Trends in the Periodic Table

Trends in the Periodic Table. Atomic Radius. Atomic radius is simply the radius of the atom, an indication of the atom's volume. Atomic radius is one-half the distance between the two nuclei in a molecule consisting of two identical atoms. Trends in Atomic Size cont.

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Chem 11

Even More on Periodic Trends. Chem 11. Ionization Energy. Ionization Energy. The amount of energy required to completely remove an electron from a gaseous atom. Removing one electron makes a +1 ion. The energy required to remove one e - is called the first ionization energy.

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History of the Periodic Table

History of the Periodic Table. Dmitri Mendeleev - Arranged all the known elements by atomic mass. - Noticed that the similarities in their chemical properties appeared at regular intervals (periodic). - Moved elements into different groups if they had similar properties.

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Periodic Trends

Periodic Trends. Reactivity of Active Metals. Active metals become more reactive as you go down a group. Ionization Energy. Energy required to remove the most loosely held electron from an atom The greater the ionization energy, the more strongly the atom holds onto its electrons

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