Polar & non-polar covalent bonds

Slides:



Advertisements
Similar presentations
bond formed by the giving or Ionic Bond bond formed by the giving or taking of electrons.
Advertisements

What is a Chemical Bond? A chemical bond is a force holding two or more atoms together to form a molecule.
Valence electrons are important because…  They are the electrons in the outermost shell  They are the same for each element in a group (column).  Want.
It’s another WEINERPOINT PRESENTATION PART III Polar Bonds.
Inorganic Chemistry – Chemical Bonding. Chemical Bonding (1). When two or more atoms react ---  chemical bond – Valence electrons – Form Ionic bonds.
Valence Electrons and Bonding
Chemical Bonding. Chemical Bond The forces that hold groups of atoms together and make them function as a unit Bonding involves only the valence electrons.
  In covalent bonding, the two electrons shared by the atoms are attracted to the nucleus of both atoms. Neither atom completely loses or gains electrons.
Chapter 5 Section 3 Notes The chemical bond formed when two atoms share electrons is called a covalent bond. Except for noble gases, nonmetals can bond.
 Obj:  You will be able to describe the types of chemical bonds & how they form.  Do Now: In your own words, define a bond?  Please take out pH Lab.
Ionic & Covalent Bonding Electronegativity & Polarity.
Homonuclear & Heteronuclear bonds Homonuclear bondsHetronuclear bonds Ethane (C 2 H 6 ) Hydrazine (N 2 H 4 ) Hydrogen peroxide (H 2 O 2 )
Covalent Bonding What is a covalent bond?. Covalent Bonding What is a covalent bond? How is a covalent bond different from an ionic bond?
1.4 Chemistry Basics Part I SBI3C Mrs. Jones. Chemistry Basics  Biology is the study of living things  All living matter is composed of chemical substances.
What you’ve learned so far…..  Atoms form bonds in more than one way  In IONIC bonding, atoms give up or gain electrons  In COVALENT bonding, atoms.
Valence Electrons: the electron(s) in the outer shell of an atom’s electron cloud, which can combine with other atoms to form molecules *The number.
8th 4.2 Ionic and Covalent Bonds
Types of Chemical Bonds
Polarity of Covalent Bonds
Solution Chemistry Unit 10 Chapter 16.
O STRUCTURE OF WATER 1 molecule of water is
Homonuclear & Heteronuclear bonds
II. Kinds of Chemical Bonds (p )
Chemistry of Life Properties of Water.
SBI4U BIOCHEMISTRY Atoms, Bonding & Molecular Polarity.
Unit 2: Biochemistry 2.2 Chemical Bonding.
Polarity and Intermolecular Forces
The unequal distribution of electrons makes
Electronegativity and Polarity
Chemical Bonds Section 2.3.
Chemical (Intramolecular) Bonding
Ionic Vs Covalent bonds
Polar and Nonpolar Cl H -Electronegativity is the ability of an atom to pull or attract electrons shared between two atoms -An atom.
Bonding continued.
Unit 1B - Matter & Qualitative Analysis SCH3u/4C
Polarity of Molecules October 2016.
Electronegativity and Polarity
Unit 2: Ecology 2.4 Chemical Bonding.
Chapter 12 Chemical Bonding
Chemistry of Life Properties of Water.
Chapter 12 Covalent Bonding
Bonding.
Chapter 12 Chemical Bonding
Class Notes 2-2 Water and Solutions.
Chapter 20 Section 2: Types of Bonds
H2O.
Chemical Bonding SCH4C Ms. Richardson.
Objectives Describe how a compound differs from an element.
What do these pictures have in common?
Types of covalent bonds
Aim: How to describe the polarity of bonds and molecules
Chemistry Review.
8th 4.2 Ionic and Covalent Bonds
VI. Polarity.
I. Why Atoms Combine Chemical Formulas Chemical Bonds Stability
Electronegativity and Polarity
Chemical Bond Forms when 2 or more atoms rearrange valence electrons to increase stability Electrical.
II. Kinds of Chemical Bonds Ionic Bond Covalent Bond Comparison Chart
Chemical Formulas and Chemical Bonding
Chemical Bonds.
Bonding, Polarity, Solubility
Bonding.
II. Kinds of Chemical Bonds Ionic Bond Covalent Bond Comparison Chart
Polar & non-polar covalent bonds
Chemical Bonds 18.2.
BOND & polarity.
Electronegativity and Polarity
Polarity and Intermolecular Forces
ionic, covalent, and metallic
Ion An ion is an atom or molecule which has gained or lost electrons making it charged, either positively or negatively. ***Protons are never lost or gained.
Presentation transcript:

Polar & non-polar covalent bonds animations

Expectation 5 Electronegativity: decides who “wins” the fight over bonding atoms. The difference in electronegativity between atoms decides the type of bond.

Electronegativity & bond type (expectation 5) The attraction to a bonding electron The difference in electronegativity decides the type of bond. Ionic bond: Difference is > 2.0 (between metals & non-metals) & results in ions due to electron transfer. Polar covalent: Difference is > 0.4 but < 2.0 & results in unequal sharing Non-polar covalent: difference is < 0.4 & allows equal sharing

Covalent bonds (Expectation 7) When electronegativity values are high, each atom fights to keep the electrons so they must share electrons to satisfy the octet rule. A covalent bond is when atoms share electrons & stay together because both have ownership over the electrons. There are 2 types of covalent bonds.

Non-polar bonding (expectation 7) Small or no difference in electronegativity results in atoms sharing electrons equally No + or – exist. They do not have to both be the same atom to be non-polar.

Polar covalent bonds (expectation 7) The atom with greater electronegativity pulls the shared electrons closer to it, resulting in unequal sharing. Eg. Cl-F The F atom is slightly negative ( ) because the electrons are closer to F. The Cl atom is slightly positive ( ) because the electrons are farther from Cl. Unequal sharing of electrons produces partial charges (poles: opposite charged ends).

Polarity (Expectation 10) Polarity exists if a molecule has charged poles (opposite ends) due to electronegativity differences These molecules are attracted to other molecules with a charge. The more similar the polarities are the easier the two substances mix.

Polarity & shape A molecule can have polar bonds & be a polar molecule. Eg. Which atom is sort of negative & sort of positive?  S-O H-Cl C-O  A molecule can have a polar bond & NOT be a polar molecule.  Eg. CO2 looks like O-C-O  Both oxygens pull equally & cancel each other out so there is no polar end.  The shape of a molecule can affect whether a molecule is polar. Polar bonds can cancel each other out.

Memorize Salt (NaCl) is ionic. Water is polar. Oil is non-polar. Ionic compounds (salt) can dissolve in polar substances (water).

Ionics dissolve in water The polarity of water explains the fact that ionic compounds dissolve in water. The charges of the ions in the ionic bond are attracted to the polar ends of water (the “sort of” negative & “sort of” positive charges).

Ionic Large electronegativity difference results in one atom taking the electron. MgO Oxygen’s has a high electronegativity & Mg is low. Bonding electron distribution Mg is + & O is – so they stick together