1. Atoms are the smallest form of elements

2.  Elements get their names in different ways unique symbol  Each element has its own unique symbol new element  Capital letter indicates a new element

3.  John Dalton (Atomic Theory)  John Dalton (Atomic Theory) said that each element is made of tiny particles called “atoms” IDENTICAL  All of the atoms of a particular element are IDENTICAL but are different from atoms of other elements

4.  Subatomic Particles found in the atom NameChargeLocationRelative Mass ProtonpositiveInside nucleus 2000 ElectronnegativeOutside nucleus-orbit the nucleus 1 Way smaller than protons or neutrons NeutronNo chargeInside nucleus 2000

5.  Positively charged nucleus  Contains neutrons and protons  Neutrons have no charge so overall charge for nucleus is positive

6.  The IDENTITY of an atoms is determined by the number of protons in the nucleus  Atomic Number-  Atomic Number- the number of protons in the nucleus

7.  TOTAL number of Protons and Neutrons in the atom’s nucleus

8. Atomic Number Atomic Mass Atomic number equals the number of protons or electrons Atomic mass equals the number of neutrons + protons.

11.  Atom correctly modeled  Correct number of subatomic particles  Correct location of subatomic particles  Includes Key  Items used to demonstrate creativity (not just colored on the page)  Atom square includes atomic mass, number and symbol  Correct energy levels and electrons in each

15.  BoronNeon

16.  HeliumCarbon

17.  Finish rest of page 34 and 35  Use your periodic table to find out if the element is a solid, liquid or gas !  We’ll grade and check it tomorrow

18.  Dmitri Mendeleev- 1869  Shows a periodic or repeating pattern of properties of the elements  Gaps- new elements discovered would complete the chart

19.  Elements arranged by atomic number (number of protons)  Each square gives specific information about the atoms of an element 1. Number at top of the square, # of protons in the nucleus of that atom 2. Chemical Symbol- abbreviation for element’s name; contains one or two letters

20.  Some elements that have not been named are given a temporary 3 letter symbol  Name of the element is written below the symbol  The number below the symbol tells the average atomic mass of all the elements

21. symbol  The color of the element’s symbol tells the physical state at room temperature.  White letters like H (hydrogen) indicate a gas  Blue letters indicate a liquid  Black letters indicate a solid

22.  Background colors of the square indicates whether the element is a metal, non-metal or metalloid.

23.  Each column (top to bottom) is called a group. similar chemical and physical properties  Elements in a group share similar chemical and physical properties  Groups are read from top to bottom  The groups are labeled at the top of the column  Group are also called “FAMILIES”

24. row  Each row of the periodic table is called a period left to right  Read from left to right  Horizontal row

25.  Three main regions  Metals on the left  Nonmetals on the right (except hydrogen)  Metalloid between

26. element’s location  The element’s location on the table tells us how reactive an element is  Reactive  Reactive - how likely an element is to undergo a chemical change  Atoms in groups 1 and 17 are the most reactive  Elements in group 18 are the least reactive

27.  Energy Superhighway Can hold 18 electrons Energy Freeway Can hold 8 electrons Energy Street Can hold 2 electrons

31.  Most elements are metals  Metals conduct electricity and heat well and have a shiny appearance  Can be shaped easily by pounding, bending, or being drawn into a long wire

32.  Group 1  Alkali metals  Ex: Sodium and Potassium  Group 2  Alkali earth metals  Less reactive

33.  Atoms of certain elements ALWAYS have the same number of protons, may not always have the same number of NEUTRONS.  Not all atoms of an element have the same MASS NUMBER  Ex: Chlorine- some have 17 protons and 18 neutrons, other chlorine atoms have 20 neutrons

34.  Sodium – 11 electrons, loses an electron  Chlorine- 17 electrons, gains an electron