Chapter 11 Introduction to Atoms

An atom is the smallest particle into which an element can be divided and still be the same substance. See timeline handout for the development of the model of the atom. Identify atom models of Thomson, Rutherford, Bohr, and the Modern Model.

What do I need to know? Know the scientist their contribution to the developing model of an atom (their experiment) their atom model!

Structure of the atom The atom contains a nucleus surrounded by one or more electrons The nucleus contains protons and neutrons. Draw an atom here (Page 320)

Structure of the atom nucleus energy level

Particle Charge Location

Particle Charge Location Proton

Particle Charge Location Proton Positive (+)

Particle Charge Location Proton Positive (+) Inside nucleus

Particle Charge Location Proton Positive (+) Inside nucleus Neutron

Particle Charge Location Proton Positive (+) Inside nucleus Neutron Neutral

Particle Charge Location Proton Positive (+) Inside nucleus Neutron Neutral

Particle Charge Location Proton Positive (+) Inside nucleus Neutron Neutral Electron

Particle Charge Location Proton Positive (+) Inside nucleus Neutron Neutral Electron Negative (-)

Particle Charge Location Proton Positive (+) Inside nucleus Neutron Neutral Electron Negative (-) Outside nucleus

Terms to copy in notes: atomic number – the number of protons in the nucleus of an atom. (*The number of protons identifies an element!) atomic mass – the average mass of one atom of an element. atomic mass unit (amu) – a measurement of the mass of one proton or one neutron.

Chemical Symbols Hydrogen symbol is H Cobalt symbol is Co A chemical symbol is one or two letter(s) representing an element. If the symbol is one letter, it is a printed capital. Hydrogen symbol is H If two letters, the first is a printed capital and second is lower case. Cobalt symbol is Co

Know the Following Elements! The first 20 elements and symbols, plus 7 others, must be properly identified together. iron copper silver gold mercury tin lead The symbols must be written in correct form. Spelling counts!

Electrons Electrons are located in an electron cloud around the nucleus. There are different energy levels (“orbits” in the Bohr model) that electrons fill. 1st energy level can hold 2 electrons 2nd can hold 8 electrons 3rd can hold 18 electrons 4th can hold 32 electrons

Energy Levels of carbon atom

Fe Today’s periodic table is based on atomic number. Each element’s square contains: atomic number (protons) chemical symbol element name atomic mass (protons & neutrons) This is an average 26 Fe Iron 55.847

How to find the number of neutrons in an atom Round the atomic mass to the nearest whole number. Subtract the number of protons (atomic number). The difference is the number of neutrons. boron 10.81 atomic mass (protons + neutrons) 11 rounded - 5 atomic number (protons) 6 neutrons

Aluminum atomic mass rounded - atomic number neutrons

Practice calculating the number of neutrons in an atom Number a blank sheet of paper 1 to 10. Write the name for each element from the periodic table for elements 1-10. Use the right side of your paper to calculate the number of neutrons for elements 1-10. Write your answer next to the elements name.

Gaining or losing a neutron makes an atom an isotope. Isotopes are still the same element, just more or less neutrons. carbon 12 has 6 neutrons (always 6 protons) carbon 14 has 8 neutrons (always 6 protons) The 12 refers to the mass number (protons + neutrons)

Valence electrons are electrons farthest away Valence electrons are electrons farthest away from the nucleus (outer energy level). - involved with chemical reactions. - gives an atom its chemical characteristics. - can be shared, or transferred. - Atoms with a full valence energy level are most stable (less reactive).

hydrogen oxygen carbon neon electron dot diagram – represents the valence electrons of an element. - uses an element symbol surrounded by dots representing valence electrons. H O C Ne hydrogen oxygen carbon neon

The Periodic Table of Elements Chapter 12 Notes The Periodic Table of Elements In 1869 a Russian scientist Dmitri Mendeleev arranged elements in order of increasing atomic mass, and chemical properties. He used his table to predict properties of elements not yet discovered!

Fe Today’s periodic table is based on atomic number! Each element’s square contains: atomic number (protons) chemical symbol element name atomic mass (protons & neutrons) This is an average 26 Fe Iron 55.847

An element’s properties can be predicted by its location on the periodic table. Groups or families: vertical columns numbered 1-18. elements have similar properties Periods: across rows numbered 1-7 elements have predictably different patterns.

Metals Metals are found to the left of the stair step. Physical properties: Hardness Shininess (luster) Malleability (pound into shapes) Ductility (drawn out into a wire) Good conductors Magnetic (Co, Ni, Fe) Mostly solids at room temp.

Metals Chemical properties: wide range Some violently react with water (Na, K) Some unreactive (Au, Cr) Some corrode (react slowly with O2 and flake off) Alloys (mixture of metals) bronze (Cu + Sn) stainless steel

Metals Elements are increasingly nonmetallic reading left to right. Tend to lose electrons forming positive ions (1+, 2+) Alkali Metals Group 1 (1 valence electron) Most reactive metals! Very soft & shiny

Metals Alkaline Earth Metals Group 2 (2 valence electrons) Not as reactive as Group 1 but more reactive than most metals. Fairly hard, grey-white color Good conductors of electricity

Metals Transition Metals Groups 3-12 Fairly stable, react slowly with H2O Similar reactivity between columns Hard and shiny Good conductors of electricity

Metals Lanthanides and Actinides Called rare earth metals Fit in Periods 6 and 7 between alkaline earth metals and the transition metals. Placed below periodic table for convenience. Soft, malleable, shiny, very conductive

Nonmetals Located right of the stair step Physical properties: Most are gases at room temp. (low boiling point). dull brittle lower densities poor conductors of heat & electricity

Nonmetals Halogen Family Chemical properties: Most readily form compounds Will take electrons from metals forming negative ions (1-, 2-) Will also share electrons Many form diatomic molecules (O2, N2, H2) Halogen Family Group 17 (7 valence electrons) Very reactive! Dangerous to humans

Nonmetals Noble Gases Hydrogen Group 18 Chemically stable (unreactive) Do not gain, lose, or share valence electrons Hydrogen Alone in upper left corner Simplest element Not grouped in a family

Metalloids Along the stair step (7 elements) Have some properties of metals & nonmetals Used to make semiconductors