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Chapter 7.  1 st developed by Dmitri Mendeleev (Russia) & Lothar Meyer (Germany) on the basis of the similarity in chemical and physical properties 

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Presentation on theme: "Chapter 7.  1 st developed by Dmitri Mendeleev (Russia) & Lothar Meyer (Germany) on the basis of the similarity in chemical and physical properties "— Presentation transcript:

1 Chapter 7

2  1 st developed by Dmitri Mendeleev (Russia) & Lothar Meyer (Germany) on the basis of the similarity in chemical and physical properties  Mendeleev … ◦ started by organizing elements by increasing mass. ◦ Recognized a repetition of pattern. ◦ Placed elements by same column  same properties ◦ Predicted correctly about the existence of new elements  Henry Moseley ◦ established that each element has a unique atomic number, which added more order to the periodic table ◦ Identified the atomic number with the # of protons in the nucleus of the atom & the # of electrons in the atom.

3  Atoms aren’t hard spheres with well-defined shells of electrons  The edges of atoms are a bit “fuzzy”  The quantum mechanical model of the atom supports the notion of electron shells: certain distances from the nucleus at which there is a higher likelihood of finding an electron

4  The size of an atom can be gauged by its bonding atomic radius, based on measurements of the distances separating atoms in their chemical combinations with other atoms  Measure the atomic radius from the center of the nucleus to the outermost electron. 1) Atom size increases going down a group. 2) Atomic size decreases going left to right across the period.

5  Ionization energy – the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion  1 st ionization energy (I 1 ) – The energy needed to remove the first electron from a neutral atom, forming a cation  2 nd ionization energy (I 2 ) – the energy needed to remove the second electron  The greater the ionization energy, the harder it is to remove an electron

6  HIGH ionization energy means the atom hold onto the electron tightly and a lot of energy is need to pull it off  LOW ionization energy means the atom holds onto the electron loosely so breaking it apart doesn’t require much energy

7 Periodic Trends in Ionization Energies  Ionization energy decreases as you move down a group.  Ionization energy increases as you move from left to right on the periodic table.  Representative elements show a larger range of values of I 1 than do the transition metal elements


9  Electron affinity – the energy change that occurs when an electron is added to as gaseous atom  A negative electron affinity = the anion is stable  A positive electron affinity = the anion is higher in energy than are the separated atom and electron. The anion is not stable and will not form

10  If the electron affinity is negative, the atom releases energy.  Normally, non-metals have a more negative electron affinity than metals. The exception is the noble gases.

11  Election affinities become more negative as we proceed from left to right  Halogens have the most negative electron affinities  The electron affinities of the noble gases are all positive since the added electron would have to occupy a new, higher-energy subshell  Electron affinity doesn’t change greatly as we move down a group. Electron affinity should become more positive (less energy released).


13 MetalsNon-Metals Have a shiny luster; various colors, although most are silvery Do not have a luster; various colors Solids are malleable and ductile Solids are usually brittle; some are hard, and some are soft Good conductors of heat and electricity Poor conductors of heat and electricity Most metal oxides are ionic solids that are basic Most non-metallic oxides are molecular substances that form acidic solutions Tend for form cations in aqueous solutions Tend to form anions or oxyanions in aqueous solution Pg Table 7.3 Characteristic Properties of Metals and Nonmetals

14  Metallic Character - The tendency of an element to exhibit properties of metals  Metallic character generally increases going down a column and decreases going from left to right across a period

15  Metals conduct heat & electricity  They are malleable & ductile  Solids at room temp. except mercury(Hg) (it’s liquid)  Melt at very high temps  Have low ionization energies & are consequently oxidized (lose electrons) when they undergo chemical reaction.  Many transition metals have the ability to form more than one positive ion.

16  metal oxide + water  metal hydroxide ◦ Most metal oxides are known as basic oxides ◦ Ex: Na 2 O (s) + H 2 O(l)  2NaOH (aq)  metal oxide + acid  salt + water ◦ Ex: MgO (s) + 2HCl (aq)  MgCl 2 (aq) + H 2 0 (l)

17  Not lustrous & generally are poor conductors of heat and electricity  Non-metals commonly gain enough electrons to fill their outer p sub-shell completely, giving a noble gas electron configuration.  Molecular substances - Compounds composed entirely of nonmetals ◦ Ex: oxides, halides, and hydrides  Melting points are gen. lower than those of metals

18  Nonmetal oxide + water → acid ◦ Most nonmetal oxides are acidic oxides ◦ CO 2 (g) + H 2 O (l)  H 2 CO 3 (aq)  Nonmetal oxide + base  salt + water ◦ CO 2 (g) + 2NaOH (aq)  Na 2 CO 3 (aq) + H 2 O (l)

19  Have properties that are intermediate between those of metals and nonmetals

20 Group 1A: The Alkali Metals Characteristics ◦ Soft metallic solids ◦ Silvery ◦ metallic luster ◦ high thermal and electrical conductivities ◦ Low densities and melting points ◦ Most active metals ◦ Exist in nature only as compounds

21 Group 2A: Alkaline Earth Metals  Solids with typical metallic properties  Harder, more dense, and melt at higher temperatures when compared to alkali metals  Very reactive towards nonmetals, but not as reactive as alkali metals  Both alkali and alkaline earth metals react with hydrogen to form ionic substances that contain the hydride ion, H -

22 Hydrogen  Hydrogen is a nonmetal with properties that are distinct from any of the groups of the periodic table  It forms molecular compounds with other nonmetals, such as oxygen and the halogens

23 Group 6A: The Oxygen Group  Most important element in group 6A  Exists in several allotropic forms (different forms of the same element in the same state)  Oxygen is encountered in two molecular forms, O 2 (common form) and O 3 (aka ozone)  Oxygen has a strong tendency to gain electrons from other elements, thus oxidizing them  In combination with metals, oxygen is usually found as the oxide ion, O 2-, although salts of the peroxide ion, O 2 2-, and superoxide ion, O 2 -, are sometimes formed

24 Sulfur!!  2 nd more important element in group 6A  Also exists in several allotropic forms  Elemental sulfur is more commonly found as S 8 molecules  In combination with metals, it is more often found as the sulfide ion, S 2-

25  Nonmetals that exist as diatomic molecules  There melting and boiling points increase as you go down the column  Have the most negative electron affinities of the elements  Their chemistry is dominated by a tendency to form 1- ions, especially in reactions with metals

26  Group 8A: The Noble Gases aka inert gases  Nonmetals that exist as monoatomic gases  Very unreactive since they have completely filled s and p subshells. Have the complete octet  Have large 1 st ionization energies  Only the heaviest noble gases are known to form compounds, and they do so only with very active nonmetals, like fluorine

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