Pure Substances Made of only one kind of matter and has definite properties. Elements: Cannot be broken down into other substances by any physical or
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1 Periodic Table
2 Pure Substances Made of only one kind of matter and has definite properties. Elements: Cannot be broken down into other substances by any physical or chemical means. Compounds: A substance made of 2 or more elements that are chemically combined. Examples: water, carbon dioxide
3 Particles of Matter Atom is the smallest particle of an element. Atomic Theory: John Dalton formed the basis of our understanding of atoms. Molecule: Basic particle of a compound. A group of atoms that are joined together and act as a single unit.
4 Structure of an Atom Nucleus central core of the atom. Contains protons + neutrons. Protons: positive Neutrons: no charge Electrons: negative, move around nucleus. Atoms are neutral because protons and electrons are equal.
5 Atoms Most of the mass is in the nucleus. Most of the volume is in the space where the electrons move. Not all electrons are the same distance from the nucleus and don t t have equal strength. Valence electrons: The electrons that are the farthest away or most loosely held. # of valence electrons determines many properties of the atom (element)
6 Periodic Table Mendeleev recognized a hidden pattern in the elements. Wrote facts about properties. Noticed patterns when elements were arranged in increasing atomic mass.
7 Periodic Table Atomic Mass The average mass of 1 atom of the element. Protons = 1amu Neutrons = 1amu Electrons = 0 amu Atomic Number The # of protons in the nucleus. Identifies the element Periodic Table is arranged by atomic number.
8 Periodic Table Atomic number Chemical Symbol Name Atomic Mass
9 Groups Elements in a column Families Group Family name based on 1 st element in the column. Similar Characteristics Have same number and arrangement of valence electrons.
10 Periods Horizontal rows Elements from different families Not similar properties Last element an inactive gas Reactive unreactive 7 periods Valance electrons increase from left to right across a period.
11 Bohr Diagram Suggested electrons moved in a set path. Each electron has a certain energy that is determined by its path. Must gain energy to move to a higher energy level.
12 Lewis Structure The chemical symbol for the element is surrounded by the number of valence electrons present in the ion. Atoms will gain or lose electrons in order to achieve a stable, Noble Gas (Group VIII), electronic configuration. Negative ions (anions) are formed when an atom gains electrons. Positive ions (cations) are formed when an atom loses electrons
13 Electron Shells 1 st shell: 2 Electrons 2 nd Shell: 8 electrons 3 rd Shell: up to 18 electrons, although considered full if it has 8 electrons
14 Metals Physical Properties Hardness Shiny Malleable Ductile Good Conductors Magnetic Most solid at room temp.
15 Metals: Chemical Properties Reactivity: Varies among metals Metals in a group have similar properties and change gradually across the table
16 Alkali Metals Group 1 So reactive never found uncombined in nature. Soft, shiny Only 1 electron in outer shell
17 Alkaline Earth Metals Group 2 Reactive but less reactive than group 1. Hard Good Conductors 2 Valence electrons
18 Transition Metals Group So similar to each other that the difference between columns is hard to detect. Hard. Shiny Good conductors Fairly Stable
19 Metals in Mixed Groups Group Contains metals, nonmetals and metalloids Not as reactive Lanthanides and Actinides: rare earth metals. Fit between periods 6 and 7. Lanthanides: soft, shiny, malleable, good conductors Actinides: Th and U natural the rest are artificial (synthetic), unstable
20 Nonmetals Lack properties of most metals. Located to the right of the zig zag line in table.
21 Physical Properties - NonMetals Gases at room temperature Low boiling points Dull Brittle Lower densities Poor conductors
22 Chemical Properties - NonMetals Most readily form compounds Group 18 no because they don t t gain or lose valance electrons. Nonmetal can combine with metals. Example: Salt Nonmetals can combine with other nonmetals by sharing electrons
23 Families of Nonmetals Carbon Family Group 14 4 valence electrons 1 nonmetal 2 metalloids 2 metals Nitrogen Family Group 15 5 valence electrons 2 nonmetals 2 metalloids 1 metal
24 Families of Nonmetals Oxygen Family Group 16 6 valence electrons Gains/shares 2 electrons when it reacts 3 nonmetals 1 metalloid 1 metal Halogen Family Group 17 All metals but 1 7 valence electrons Gain/share 1 electron Very reactive
25 Families of Nonmetals Noble Gases Group 18 8 valence electrons Don t t gain/share/lose electrons Chemically stable Unreactive Hydrogen Simplest element Chemical properties differ from all other elements
26 Metalloids On the border between metals and nonmetals Some characteristics of metals and nonmetals Si the most common Vary in conducting electricity
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