Bellringer 9/27 Write the Bohr model for Calcium

Periodic Table Periodic Table – arrangement of elements in order of increasing atomic number with elements having similar properties in vertical columns Groups – vertical columns Periods – horizontal rows

ALKALI METALS Group 1 Hydrogen is not a member, it is a non-metal 1 electron in the outer shell Soft and silvery metals Very reactive, esp. with water Conduct electricity Image:

ALKALINE EARTH METALS Group 2 2 electrons in the outer shell White and malleable Reactive, but less than Alkali metals Conduct electricity

TRANSITION METALS Groups in the middle Good conductors of heat and electricity. Some are used for jewelry. The transition metals are able to put up to 32 electrons in their second to last shell. Can bond with many elements in a variety of shapes.

BORON FAMILY Group 3 3 electrons in the outer shell Most are metals Boron is a metalloid

CARBON FAMILY Group 4 4 electrons in the outer shell Contains metals, metalloids, and a non-metal Carbon (C)

NITROGEN FAMILY Group 5 5 electrons in the outer shell Can share electrons to form compounds Contains metals, metalloids, and non-metals

OXYGEN FAMILY Group 6 6 electrons in the outer shell Contains metals, metalloids, and non-metals Reactive

Halogens Group 7 7 electrons in the outer shell All are non-metals Very reactive are often bonded with elements from Group 1

Noble Gases Group 8 Exist as gases Non-metals 8 electrons in the outer shell = Full Helium (He) has only 2 electrons in the outer shell = Full Not reactive with other elements

Rare Earth Metals Some are Radioactive The rare earths are silver, silvery- white, or gray metals. Conduct electricity

Groups Representative elements – group A elements Transition elements – group B elements Lanthanide and actinide series = inner transition metals

Groups (reminder) The group = number of valence electrons that the element has Valence electrons are electrons in the outermost shell of the atom All group 1A elements have 1 valence electron. Likewise, all group 8A elements have 8 valence electrons.

Charges Every element wants 8 valence electrons to become stable. They will gain or lose valence electrons to form an octet For example…Group 1A elements have 1 valence electron. They can either gain 7 electrons to have an octet or lose 1. What is easier? Lose 1 If an element loses 1 electron (1 negative charge) what charge will the resulting ion have? +1

Oxidation numbers The charge an element would have if it released or obtained electrons to look like a noble gas. Metals release electrons Nonmetals obtain electrons

Characteristics Elements in the same group exhibit similar chemical characteristics due to the fact that they all have the same number of valence electrons. The most stable number of valence electrons is 8 called an octet

Predict the oxidation numbers for the following A. Al B. Mg C. N D. Na E. Cl

Physical States and Classes of the Elements Majority of the elements are metals. They occupy the entire left side and center of the periodic table. Nonmetals occupy the upper-right-hand corner. Metalloids are located along the boundary between metals and nonmetals

Metals elements that have luster, conduct heat and electricity, and usually bend without breaking.

Transition Metals The elements in Groups 3 through 12 of the periodic table are called the transition elements. All transition elements are metals. Many transition metals can have more than one charge

Inner Transition Metals In the periodic table, two series of elements, atomic numbers and , are placed below the main body of the table. These elements are separated from the main table because putting them in their proper position would make the table very wide. The elements in these two series are known as the inner transition elements.

Inner Transition Metals Lanthanides First series of inner transition element follow element number 57, lanthanum. actinides, 2 nd series of inner transition elements have atomic numbers ranging from 90 (thorium, Th) to 103 (lawrencium, Lr).

Non Metals Although the majority of the elements in the periodic table are metals, many nonmetals are abundant in nature Most nonmetals don’t conduct electricity, are much poorer conductors of heat than metals, brittle when solid. Many are gases at room temperature; those that are solids lack the luster of metals.

Properties of Metals and Nonmetals

Metalloids have some chemical and physical properties of metals and other properties of nonmetals. In the periodic table, the metalloids lie along the border between metals and nonmetals.

Bellringer 9/28 Given: iodine, helium, sulfur, or hydrogen, which is a halogen?

Periodic Trends Periodic Trends are trends that occur across the periodic table and down the periodic table They include: atomic radius, Ionization energy, electro negativity, metallic character ionic radius

Atomic Radius Atomic Radius – size of the atom  Increases  Decreases

Atomic radius The distance from the outer edge of the electron cloud to the nucleus. The radius increases as the principle quantum number increases. So elements increase going from top to bottom. The period they are in increased, radius increases.

As you move from left to right across the period things change. The # of protons in the nucleus increases. This causes the electrons to be attracted to the nucleus more and the size of the elements decrease. As you move from left to right radius decreases.

Which element in the pair is larger? A. Sn, Sr B. Cl, I C. S,P D. Ac, U E. Na, Rb F. B, Al

Determining the Atomic Radius of a Nonmetal (Chlorine) Click in this box to enter notes. Copyright © Houghton Mifflin Company. All rights reserved. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.]

Determining the Atomic Radius of a Metal (Molybdenum) Click in this box to enter notes. Copyright © Houghton Mifflin Company. All rights reserved. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.]

Ionization Energy Ionization energy – the ability to pull off 1 electron Increases  Decreases 

Ionization energy The energy required to remove the most loosely held electron from an element. Large radii elements lose electrons easily Small radii elements require energy to remove electrons.

Metals- don’t like electrons lose them easily Nonmetals – like electrons, want to keep them, require energy to remove them.

Electro negativity Electro negativity – the ability of an atom to attract another atom Decreases  Increases 

Metallic Character Metallic character – how much like a metal the element is Increases  Decreases 

Electron affinity The ability of an atom to attract electrons to itself. Metal = low affinity Nonmetals = high affinity Large radius = low affinity Small radius – high affinity

Metals and nonmetals Metals tend to lose electrons. Nonmetals tend to gain electrons. The goal is to get enough electrons in the outer energy level to look like a noble gas. Every electron lost leaves behind a net + charge.

Energy electron gained causes a net – charge. These charges effect the radius of the elements. Elements with charges are called ions

Ionic radius The more + charge an ion has the greater the ability to attract electrons to itself and is therefore smaller. The more – charge an ion has the more electrons it has pulling away from the nucleus and therefore they are larger.

Ionic Radius When you talk about ionic radius, you are comparing an atom and its ion When an atom has a negative charge, you have added electrons Which makes it bigger For example, which will be larger: Cl or Cl -1

Ionic Radius When an atom has a positive charge, you have taken away electrons Which makes it smaller For example, which will be larger: Na or Na +1

Which is larger? A. Ca, Ca +2 B. Cl, Cl - C. Br -, F - D. Pb, Pb +4

Periodic Table Trends Click in this box to enter notes. Copyright © Houghton Mifflin Company. All rights reserved. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.]

Ionic Radii Copyright © Houghton Mifflin Company. All rights reserved. Click in this box to enter notes. Copyright © Houghton Mifflin Company. All rights reserved. Go to Slide Show View (press F5) to play the video or animation. (To exit, press Esc.) This media requires PowerPoint® 2000 (or newer) and the Macromedia Flash Player (7 or higher). [To delete this message, click inside the box, click the border of the box, and then press delete.]