Atoms, first Periodic Table, second MT 1 Review Atoms, first Periodic Table, second

What is the central part of the atom called? Review Questions What is the central part of the atom called? What is the most dense part of an atom called? What is the biggest part of the atom? What part of the atom contains most of its mass? What is the smallest part of the atom that contains the atom’s properties?

Made of Protons (+) and Neutrons (•) Positive and Neutral The NUCLEUS Made of Protons (+) and Neutrons (•) Positive and Neutral

What part of the atom does the electron cloud hold? Review Questions What part of the atom does the electron cloud hold? What is the smallest part of an atom? What part of the atom does not have a measurable mass? What part of the atom is important in atomic bonding?

Negatively charged (-) ELECTRONS Negatively charged (-)

Remember Protons – Positive (+) Electrons – Negative (–) Neutrons – Neutral (•)

Comparison If the nucleus of an atom was a marble at the starting line of a race track, a grain of sand 100 yards away would represent the first electron

Comparison Now you make one… 2 minutes

Periodic Table Vocabulary Atomic Number – # of Protons Atomic Mass – # of Protons plus Neutrons Atomic Number – # of Protons (also equal to Number of Electrons) Atomic Mass – Number of Protons and Neutrons

Periodic Table Vocabulary Atoms are neutral Valence Electrons: # of electrons in outer shell ***Important for atomic bonding Atoms are neutral Valence Electrons: # of electrons in the outer/last shell of an atom ***Important for atomic bonding

Do the rows & columns have a name?

Columns: Known as A Group or Family

Rows: Known as Periods

What do all the colors mean? Elements are arranged by increasing atomic number and atomic mass. The trend increases from left to right and from top to bottom.

What do all the colors mean? Elements are arranged based on similar properties Elements are arranged by increasing atomic number and atomic mass. The trend increases from left to right and from top to bottom.

There are 3 main groups of elements -Metals -Nonmetals -Semi-metals

Metals Shiny surface Good conductors Solids at room temperature Malleable (bendable). Shiny surface Good conductors of heat and electricity. usually solids at room temperature malleable (bendable).

Metals are YELLOW

Nonmetals dull-colored brittle Do not conduct heat or electricity.

Nonmetals are GREEN

Semimetals (Metalloids) having properties of both metals and non-metals.

Semimetals (Metalloids) are PURPULE

Groups on Periodic Table of Elements

Are there any subgroups? YES! Metals Alkali Metals Alkaline Earth Metals Transition Metals Rare Earth Metals Non-Metals Halogens Noble Gases

Alkali Metals Group 1 highly reactive 1 Valence Electron Low ionization energy & electronegativity Group 1 highly reactive 1 Valence Electron low ionization energy because they give up their 1 electron easily Giving up electrons makes these positive ions

Low ionization energy & electronegativity Alkaline Earth Metals Group 2 very reactive 2 Valence Electrons Low ionization energy & electronegativity Group 2 very reactive 2 Valence Electrons low ionization energy because they give up their 2 electrons easily Giving up electrons makes these positive ions

Transition Metals 38 elements in the middle of P.T. Metals in Group 3 to 12 Share characteristics of all metals 1 or 2 electrons in outer shell

Halogens Group 17 7 Valence Electrons High ionization energy & electronegativity Outer shell is almost full

Noble Gases Group 18 odorless and colorless Gases: 8 electrons in outer shell (FULL) No Electronegativity (don’t want additional electrons) High Ionization Energy

Groups on PT of E

PT of E TRENDS Ionization energy – how much energy REQUIRED to remove electrons from an atom Electronegativity – the pull of the nucleus on electrons (attractiveness)

PT of E TRENDS Ionization energy – how much energy REQUIRED to steal, take, remove electrons from an atom Electronegativity – the pull of the nucleus on electrons (attractiveness) Electronegativity AND Ionization Energy – Highest @ top, right of periodic table Increases moving left to right Increases moving bottom to top

PT of E TRENDS Remember: The stronger the attraction (electronegativity) electrons have to the nucleus the harder they are to remove (ionization energy) This is why they have the same trend!

PT of E TRENDS Atomic Radius/Atomic Radii– how much space an atom takes up (how big an atom is) Largest @ bottom, left of periodic table Increases moving right to left Increases moving top to bottom

Elbow Partners Turn to the person sitting next to you… Discuss… Explain how the Periodic Table of Elements organizes the atoms by their structure.

The Periodic Table of Elements organizes the atoms by their structure…. Low # of protons (Atomic #), Low atomic mass Low # of rings High # of Valence e- High # of protons (Atomic #), High atomic mass Low # of Valence e- Size increase bottom to top High IE, High EN- hard to lose e- High # of rings Low IE, Low EN- easy to lose e- Size decrease left to right-pulls atom tighter

Quick Write Take 5 minutes and answer this question in your notes Explain how the location of an atom on the Periodic Table tells a lot about that atom’s characteristics.

Explain how the location of an atom on the Periodic Table tells a lot about that atom’s characteristics. Metals Non-Metals Alkali Metals Transition Metals Noble Gases -one outer e- -very reactive -never found alone -soft & dense -2 or 1 outer e- -shiny -good conductor of heat & electricity -very useful in every day life -8 outer e- -outer ring is FULL -never connected to another atom -gases in our atmosphere