2/22 Answer IQ on Yellow half sheet

Periodic – means regular, repeated pattern. Modern Periodic table vs. Mendeleev’s Brainpop

Reading the Periodic Table - atomic #= #of protons = #electrons - element symbol -element’s name Atomic mass/weight: ave of all known masses Mass # protons + neutrons (nucleus) 26 Fe Iron

What’s the difference between Mass # & atomic #? (1:41) Mass # & atomic #? (1:41) Atomic # is equal to the number of protons or electrons (unless charged) Mass # is the # of protons PLUS the # of neutrons (each equals 1 AMU)

Drawing an atom Draw atomic structure of H & He as a class. Draw atomic structure O on your own. Determine valence e-s for each one. Building an atom

Uses the elements symbol and dots for # of val. e-s. Ex. H Complete Lewis Dot structure page on PT Basics Packet. Lewis Dot structure

Elements are arranged: Vertically into Groups Horizontally Into Periods

Periods or Rows Contains a series of elements from different families. The elements have very different properties. 7 periods of elements - 7 electron shells

If you looked at an atom from each element in a period you would see…

Each atom has the same number of electron holding shells. An example…

The period 4 atoms each have 4 electron containing shells K (Potassium) Atom Fe (Iron) Atom Kr (Krypton) Atom 4 th Shell

Groups or Families Elements in a column. Numbered 1 on left to 18 on right. Elements in a group have similar characteristics.

If you looked at one atom of every element in a group you would see…

Each atom has the same number of electrons in it’s outermost shell. An example…

The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

The number of outer or “valence” electrons in an atom effects the way an atom bonds. The way an atom bonds determines many properties of the element. This is why elements within a group usually have similar properties.

Patterns on the PT

Groups: Columns  The vertical columns (up and down)  called groups (18) or families (I- VIII)  Family # gives # of valence e-s.  Metallic character increases from top to bottom.  Share similar chemical and physical properties/looks as long as in the same column/family. Ex. Li, Na, and K have similar properties, all in 1 family. Write the val e-s for families I thru VIII on your PT

Periods: Rows (7) The horizontal rows left to right. There are 7. ‘periodic’ means repeating pattern. Per. # tells us how many energy levels the elements have. Elements in a period are not alike in properties. 3 repeated PATTERNS left to right: 1. METAL TO NONMETAL 2. HIGHLY REACTIVE TO NONREACTIVE 3. Atomic number/mass (smaller/bigger: +1 p) Val. E-s go up and affinity/attraction for electrons goes up. Vid (3 min) Vid Draw the number of shells for Periods 1 thru 7 on your PT

2/23 p. 26 Metals, Non-metals, Metalloids Answer IQ on pink half sheet.

Practice Locate the element Chlorine on your PT. Decide which 2 elements will have properties similar to those of Cl. a. S and Ar b. Br and I c. Br and F d. O and F PT Videos

Practice: Circle the element Ca on your PT. Determine and circle the 2 elements that have properties most similar to Ca.

Rows & Columns Combined OVERALL (back of PT) Metals are on the left; Non-metals are on the right. Metalloids are in between metals & non- metals, on ‘staircase’ or the “zig-zag.”

Metals and non-metals

MetalsNon-metals Conductive (heat/electrictiy)**opposite properties of metals Malleable: flattenedbrittle: shatter Ductile: stretched/rolled Dense High MP/BP Easily give away electronsGain or share electrons High luster: aka – shininessDull Ex: iron, copper, silverEx: Carbon, sulfur

Metals, non-metals, metalloids activity: Color in the appropriate section on each PT, then cut and paste the characteristics in the right category.

Metals Conductive (heat/electricity) Nonmetals silver or white in color, lustrous (shiny) dull in appearance malleable and ductilebrittle if solid Densepoor conductor of heat and electricity high melting and boiling pointslow mps and bps low densities many react with acidsdoes not react with acids all solids except, mercury (Hg)exist in all three states of matter * Metalloids are combined properties of both metals and nonmetals. * Metalloids are combined properties of both metals and nonmetals.

Some properties of metals to look at (in notebook)  Malleability- Ability to be flattened into thin sheets. Ex. Aluminum  Ductility- Ability to be drawn into wires. Ex. Copper.  Heat and electrical conductivity- Ability to allow heat and electricity to pass through. Ex. Copper (p. 306)

2/24 p. 30 Atomic BondingAtomic Bonding IQ: Green half sheet

On p. Draw the Bohr model for Sodium (Na). Then, predict what would a Na +1 ion be like.

Bonding (back of PT) 1.The # of outer/“valence” e-s in an atom affects the way an atom bonds. 2. The ‘magic #’ is 8 e - want to have 8 friends total! 3. Makes a complete outer shell, called a complete octet. 4. Group 1 elements will readily bond with Group 17 elements to form salts. Can you tell why? So, Group 2 elements will readily bond with group _________.

5) Two types of bonds: a) Covalent bond: means to share electrons. Usually between two non-metals but can happen between a metal and a non-metal. b) Ionic means to gain or lose valence e-s, usually metal with a non metal. Add: Noble gases have a complete outer shell (2 or 8e-s) so they don’t bond with anything, called inert gases. The way an atom bonds determines many properties of the element.

For example, during the reaction of sodium with chlorine: sodium (on the left) loses its one valence electron to chlorine (on the right),valence electron resulting in a positively charged sodium ion (left) and a negatively charged chlorine ion (right).ion The reaction of sodium with chlorine Concept simulation - Reenacts the reaction of sodium with chlorine. (Flash required)Flash

In notebook: A molecule is formed. Ionic (Metal and a non-metal only)- Na and Cl Na easily loses the 1 extra electron and becomes Na + while Cl readily takes the electron and becomes Cl - Formula: NaCl Video Video Covalent (non-metals only) H and H Neither atom wants to lose electrons so they share. Formula:

Bonding between Mg and Br Draw the lewis dot diagrams of Mg and Br. How many electrons can 1 Mg atom give away? How many electrons can 1 Br atom take? How many Br atoms are needed to bond with 1 Mg atom? What is the formula of the resulting molecule?

Do yourself. Draw Lewis dot structures and predict how many atoms of each kind will bond with each other: Ca and SSi and O

Periodic Table Basics due next Tuesday.

OQ: Name 2 elements that could hook up together to form a new substance. Explain why you picked them.