ATOMIC STRUCTURE S.MORRIS 2006

Warm Up Assignment#3 1/6/17 1. What is an atom? 2. Is Na (Sodium) a Metal, Non-Metal, or a Metalloid? Is Si (silicone) a Metal, Non-Metal, or a Metalloid? Which of the following is dull? Titanium Ti Carbon C Iron Fe Study for your quiz on density word problems

Bohr Model Video

HISTORY OF THE ATOM Niels Bohr 1913 studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits.

electrons are located in orbits outside the nucleus. Bohr’s Atom electrons are located in orbits outside the nucleus. Electron Cloud: all the area outside the nucleus nucleus

Protons and Neutrons are located inside the nucleus HELIUM ATOM -Orbit -Shell -Energy level proton N + - + N - neutron electron Protons and Neutrons are located inside the nucleus

e- have the smallest mass (technically none). amu: Atomic mass unit ATOMIC STRUCTURE **********Copy and memorize the chart************* Particle Charge Mass proton + charge 1amu neutron +/-No charge 1amu electron - charge 0 amu e- have the smallest mass (technically none). amu: Atomic mass unit

Draw the Atom HELIUM ATOM + - + - -Orbit -Shell -Energy level proton nucleus neutron electron Draw the Atom

ATOMIC STRUCTURE 2 Atomic number He the number of protons and/or electrons in an atom Atomic mass 4 the sum of protons and neutrons in an atom 3rd Period, put this in your notes, continue last assignment, draw the square around He

+Protons -Electrons Ex: Hydrogen 1 1 Find the number of electrons and protons in each one of the following elements: +Protons -Electrons Ex: Hydrogen 1 1 Fluorine Nitrogen Boron Chlorine Sulfur Sodium Beryllium Carbon Helium Argon Selenium

Where is an electron? Charge? Where is a Proton? Charge? Where is a Neutron? Charge? What is the name of the area outside the nucleus? Which subatomic particle has the least amount of mass? Which two subatomic particles make up most of the weight of an atom?

ATOMIC STRUCTURE Electrons are arranged in Energy Levels, Shells, or orbitals around the nucleus of an atom. first shell a maximum of 2 electrons second shell a maximum of 8 electrons third shell a maximum of 8 electrons fourth shell a maximum of 8 electrons

1. Electronic Configuration ATOMIC STRUCTURE There are two ways to represent the atomic structure of an element or compound; 1. Electronic Configuration 2. Dot & Cross Diagrams

ELECTRONIC CONFIGURATION With electronic configuration elements are represented numerically by the number of electrons in their shells and number of shells. For example; Nitrogen configuration = 2 , 5 7 2 in 1st shell 5 in 2nd shell N 2 + 5 = 7 14

1. ELECTRONIC CONFIGURATION Write the electronic configuration for the following elements; 20 11 8 Na O Ca a) b) c) 16 23 40 2,8,8,2 2,8,1 2,6 17 14 5 Cl Si B d) e) f) 11 35 28 2,8,7 2,8,4 2,3

Draw and label the following parts of the atom Warm up 1/9/17 Assignment #4 Draw and label the following parts of the atom

N DOT & CROSS DIAGRAMS Nitrogen With Dot & Cross diagrams elements and compounds are represented by Dots or Crosses to show electrons, and circles to show the shells. For example; X Nitrogen N 7 X X N X X 14 X X

Valence Electrons 2. DOT & CROSS DIAGRAMS O Cl Draw the Dot & Cross diagrams for the following elements; X 8 17 X O Cl a) b) X 35 X 16 X X X X X Cl X X X X X X X O X X X X X X X X X X Valence Electrons

Valence Electrons Electrons located in the outer shell of an atom; responsible for interactions with other elements (reactions).

Draw the Bohr Model of the first 26 elements in the periodic table, and write down the following details: Protons# Electrons# Valence electrons# 1P Valence. e=1 and 1 e-

SUMMARY The Atomic Number of an atom = number of protons in the nucleus. The Atomic Mass of an atom = number of Protons + Neutrons in the nucleus. The number of Protons = Number of Electrons. Electrons orbit the nucleus in shells. Each shell can only carry a set number of electrons.

WARM UP 1/12/17 Assignment # 5 1. Do the electronic configuration of the following atoms and classify them as Malleable, or Non-Malleable --V (Vanadium) --S (Sulfur) --Fe (Iron) 2. Which subatomic particles are responsible for the Atom’s weight? 3. Location of a Neutron?

Atoms presented in the periodic table are electrically neutral; therefore, they have the same amount of protons and electrons (They cancel each other out). Element # of Protons # of Electrons Overall Charge Mg (Magnesium) Cr (Chromium) S (Sulfur) Ne (Neon) Cl (Chloride) Na (Sodium) Li (Lithium)

} APE MAN Same Number every time. Protons Electrons Mass (Atomic Mass) Atomic Number Same Number every time. Protons Electrons MAN Mass (Atomic Mass) Atomic Number Neutrons

Lets Practice “APE” Who am I? I have: 13 Protons 8 Electrons Element’s name 13 Protons 8 Electrons 21 is my atomic number 52 Protons 13 Electrons 20 is my atomic number 33 Electrons 8 Protons 13 is my atomic number 21 electrons

---Do you see an element showing more than Once? ---Which one/ones? ---Why?

# * Lets Practice “APE” Who am I? I have: Element 13 Protons Al (Aluminum) 8 Electrons O (Oxygen) 21 is my atomic number Sc (Scandium) 52 Protons Te (Tellurium) 13 Electrons Al (Aluminum) 20 is my atomic number Ca (Calcium) 33 Electrons As (Arsenic) 8 Protons 13 is my atomic number 21 electrons # % @ = * +

MAN Lets Practice “Man” Mass (Atomic Mass) Atomic Number Neutrons Element Atomic MASS Atomic Number Neutrons S Sulfur Ca Calcium C Carbon Li Lithium As Arsenic Cl Chlorine Na Sodium MAN Mass (Atomic Mass) Atomic Number Neutrons

Copy the chart and fill in the blanks Warm Up 1/17/17 (Tuesday) Assign. #6 Copy the chart and fill in the blanks Element # of Protons # of Electrons Atomic mass # of Neutrons 16 23 20

Periodic Table H Li Periods are horizontal and determine the number of energy levels in an atom. Periods=Rows=# OF SHELLS Na K Rb Cs Fr

Find the number of shells in the following elements: 1. V 2. Ge 3. F 4. H 5. He 6. As 7. Rn 8. Ne 9. S 10.K

Groups are vertical and determine the number of valence electrons. 1=1 2=2 13=3 14=4 15=5 16=6 17=7 18=8 FOR COLUMNS 3-12 YOU NEED TO DO THE ELECTRONIC CONFIGURATION

Determine the number of Valence electrons of the following Elements: 1. Mg 2. B 3. Sc 4. Be 5. Cr 6. Kr 7. Xe 8. Te 9. S 10.Si

Elements in the same group have similar chemical and physical properties. Li Be S He Na Mg Se Ne

Which one/ones have similar Physical and Chemical properties? Li Be O He Mg Sr F Xe

REACTIVITY Most reactive groups 1 & 17 Least reactive/stable group 18

For metals, reactivity increases down a group and from right to left across a period. For nonmetals, reactivity increases up a group and from left to right across a period. Francium is the most reactive metal, and fluorine is the most reactive nonmetal.

Find the most reactive Element 1. Ne or F 2. S or Xe 3. Rb or Na 4. Ba or Mg 5. Sc or K 6. Rn or C 7. Cu or Cs 8. H or Fr 9. K or Ne 10. He or Be

7.Atoms of the same element with different amounts of neutrons are isotopes. Ex: diamond.