Chapter 4 Compounds and Molecules 4 1 Compounds

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Chapter 4 Compounds and Molecules

Chapter 4 Compounds and Molecules

4. 1 Compounds and Molecules • What are compounds? • Table salt is a

4. 1 Compounds and Molecules • What are compounds? • Table salt is a compound made of two elements, sodium and chlorine.

4. 1 Compounds and Molecules • Chemical bonds distinguish compounds from mixtures. • Chemical

4. 1 Compounds and Molecules • Chemical bonds distinguish compounds from mixtures. • Chemical Bonds- Are the attractive forces that hold different atoms or ions together in compounds • Mixtures are made of different substances that are just placed together. • A compound always has the same chemical formula.

4. 1 Compounds and Molecules • Chemical structure shows the bonding within a compound.

4. 1 Compounds and Molecules • Chemical structure shows the bonding within a compound. • Chemical Structure-the arrangement of bonded atoms or ions within a substance • Bond Length-The average distance between the nuclei of two bonded atoms • Bond Angle-The angle formed by two bonds to the same atom

4. 1 Compounds and Molecules • Some models give you an idea of bond

4. 1 Compounds and Molecules • Some models give you an idea of bond lengths and angles • Space filling models show the space occupied by atoms • Compounds with network structures are strong solids

4. 1 Compounds and Molecules • Some networks are made of bonded ions •

4. 1 Compounds and Molecules • Some networks are made of bonded ions • Some compounds are made of molecules • The strength of attractions between molecules

4. 2 Ionic and Covalent Bonds • What holds bonded atoms together? • The

4. 2 Ionic and Covalent Bonds • What holds bonded atoms together? • The outermost energy level of a bonded atom is full of electrons • Atoms bond when their valence electrons interact • Generally, atoms join to form bonds so that each atom has a full outermost energy level

4. 2 Ionic and Covalent Bonds • Bonds can bend and strech without breaking

4. 2 Ionic and Covalent Bonds • Bonds can bend and strech without breaking • Ionic Bonds- are formed between oppositely charged ions • Ionic bonds are formed by the transfer of electrons • Ionic compounds are in the form of networks, not molecules • When melted or dissolved in water, ionic compounds conduct electricity

4. 2 Ionic and Covalent Bonds • Metallic Bonds- a bond formed by the

4. 2 Ionic and Covalent Bonds • Metallic Bonds- a bond formed by the attraction between positively charged metal ions and the electrons around them • The atoms in metals like copper form metallic bonds • Covalent Bond- a bond formed when atoms share one or more pairs of electrons

4. 2 Ionic and Covalent Bonds • Atoms joined by covalent bonds share electrons

4. 2 Ionic and Covalent Bonds • Atoms joined by covalent bonds share electrons • Atoms may share more than one pair of electrons • Atoms do not always share electrons equally

4. 2 Ionic and Covalent Bonds • Polyatomic Ion- an ion made of two

4. 2 Ionic and Covalent Bonds • Polyatomic Ion- an ion made of two or more atoms that are covalently bonded and act like a single ion • There are many polyatomic ions • Parentheses group the atoms of a polyatomic ion • Some polyatomic anion names relate to their oxygen content

4. 3 Compound Names and Formulas Naming Ionic Compounds • Names of ionic compounds

4. 3 Compound Names and Formulas Naming Ionic Compounds • Names of ionic compounds include the ions of which they are composed: • The cation is listed first and is named as usual; then name the anion adding the –Ide suffix – Example: Sodium chloride • Determining the charge transition metal cation

4. 3 Compound Names and Formulas Naming covalent compounds • Name the component elements

4. 3 Compound Names and Formulas Naming covalent compounds • Name the component elements in order. • Numerical prefixes are used to name covalent compounds of two elements. Table 4. 7 pg. 126 • Example: Name N 2 O 4 • Dinitrogen tetraoxide • If there was only one atom of the first element it would not have a prefix

4. 3 Compound Names and Formulas • Empirical Formula- the simplest chemical formula of

4. 3 Compound Names and Formulas • Empirical Formula- the simplest chemical formula of a compound that tells the smallest whole-number ratio of atoms in the compound • A compound’s simplest formula is its empirical formula • Different compounds can have the same empirical formula • Molecular Formulas- a chemical formula that reports the actual numbers of atoms in the molecule of a compound

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