Standard EPS Shell Presentation

Standard EPS Shell Presentation

COMPOUNDS 16.1 Chapter Sixteen: Compounds 16.1 Chemical Bonds and Electrons 16.2 Chemical Formulas 16.3 Molecules and Carbon

Compounds Chapter 16.1 Learning Goals Infer the relationship between the number of valence electrons and the behavior of atoms. Compare and contrast ionic and

covalent bonding. Draw Lewis diagrams to represent the valence electrons of atoms. Investigation 16A Chemical Bonds

Key Question: Why do atoms form chemical bonds? 16.1 Chemical Bonds and Electrons A chemical bond forms when

atoms transfer or share electrons. A covalent bond is formed when atoms share electrons.

16.1 Chemical formulas A molecules chemical formula tells you the ratio of atoms of each element in the compound. 16.1 Ionic bonds Not all compounds are made of

molecules. Ionic bonds are bonds in which electrons are transferred from one atom to another. Sodium and chlorine form an ionic bond because the positive

sodium ion is attracted to the negative chloride ion. 16.1 Why chemical bonds It takes energy form to

separate atoms that are bonded together. The same energy is released when chemical bonds form. Atoms form bonds to reach a lower energy

state. 16.1 Reactivity In chemistry, reactive means an element readily forms chemical bonds, often releasing energy. Some elements are more reactive

than others. The closer an element is to having the same number of electrons as a noble gas, the more reactive the element is. 16.1 Valence electrons

Chemical bonds are formed only between the electrons in the highest unfilled energy level. These electrons are called valence electrons. 16.1 Valence electrons and the periodic table Going from left to right across a period

each new element has one more valence electron than the one before it. How many valence electrons does nitrogen have? 16.1 Valence electrons and

the periodic table Oxygen combines with one beryllium atom because beryllium can supply two valence electrons to give oxygen its

preferred number of 8. 16.1 Valence electrons and the periodic table Carbon has four valence electrons. Two oxygen atoms can bond with a

single carbon atom, each oxygen sharing two of carbons four valence electrons. The bonds in carbon dioxide (CO2) are double bonds because each bond involves 2 electrons. 16.1 Lewis dot diagrams

A clever way to keep track of valence electrons is to draw Lewis dot diagrams. A dot diagram shows the element symbol surrounded by one

to eight dots representing the What is the dot valence electrons. structure for

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