Related Essays

  • Lab Report Gas Chromatography

    These forces occur in every atom and molecule because of the random motions of electrons. Dipole-dipole forces is when a molecule has a permanent partial cha...

  • Intermolecular Forces Of Attraction Essay

    (Chang, 2014) There are different types of intermolecular forces. These are dipole-dipole, dipole-induced dipole, ion-induced dipole, and London dispersion ...

  • Precipitation Reactions Lab Report

    Next is dipole- dipole forces which occurs between polar molecules. After that is dipole- induced dipole, it is weaker than dipole-dipole because its occurs ...

  • Four Intermolecular Forces

    The measure of the melting/ boiling point is also a measure of how strong the attraction forces are between atoms or molecules. From the strongest to the wea...

  • How To Mold An Aluminum Foil Boat

    Covalent molecules attract each other by various intermolecular forces. These include H-bonds, dipole-dipole forces, and London dispersion

  • Sucrose Results

    The molecule with the least amount of these forces is the one with the weakest bonds,

  • Chemical Bonding Research Paper

    A compound is defined as a chemical combination of two or more elements. A chemical bond is the “glue” holding together atoms of different elements. Two type...

  • Atoms: A Valence Electron

    The octet rule states that atoms that have eight electrons in its valence shell, give it the same distribution of electrons or molecules of an atom as a nobl...

  • Exothermic Reaction Lab

    Whilst looking at a substances fixed temperature, you need to consider the properties, such as structure, molecular size and the intermolecular force. Belo...

  • Properties Of Salts And Molecules

    Both elements have the properties of salts which include soluble in water, conductive, and a relatively high melting point. Molecules and Sugar molecules are...

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off
Reading...
Front

Card Range To Study

through

image

Play button

image

Play button

image

Progress

1/50

Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

50 Cards in this Set

  • Front
  • Back
  • 3rd side (hint)
London dispersion forces
Weakest of all molecular interactions.
Attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Hydrogen Bonds
Strongest of the intermolecular forces.
Formed between the hydrogen end of one dipole and a fluorine, oxygen, or nitrogen atom on another dipole.
Hydrogen bonding always involves hydrogen.
Dipole Dipole Forces
Forces of attraction between polar molecules.
A polar molecule can induce a dipole in a non polar molecule.
Metallic bonding
Metal atoms are loosely held.
Atoms don't lose their valence electrons they release them into a sea of electrons.
Thermal and electrical conductivity due to mobile valence electrons.
Malleability and ductility.
Diatomic Molecules
Occur when any two atoms of the same element form covalent bond.
*N2 O2 H2 F2 Cl2 Br2 I2*
Dia
Sigma bond
A covalent bond resulting from the formation of a molecular orbital by the end-to-end overlap of atomic orbitals.
Pi Bond
A covalent bond resulting from the formation of a molecular orbital by side-to-side overlap of atomic orbitals along a plane perpendicular to a line connecting the nuclei of the atoms
Double Covalent Bonds
Has one sigma bond and one pi bond.
Carbon & Hydrogen = sigma
Carbon & Carbon= Pi
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
Tetrahedral
AB4
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
Tetrahedral
AB4
VSPER code
Trigonal Pyramidal
AB3E
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
Tetrahedral
AB4
VSPER code
Trigonal Pyramidal
AB3E
VSPER code
Bent
AB3E2
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
Tetrahedral
AB4
VSPER code
Trigonal Pyramidal
AB3E
VSPER code
Bent
AB3E2
VSPER code
Trigonal Bipyramidal
AB5
VSPER code
A is the central atom
B is the outside atoms
E is the lone pairs on the central atom
VSPER code
Linear
AB or AB2
VSPER code
Trigonal Planar
AB3
VSPER code
Tetrahedral
AB4
VSPER code
Trigonal Pyramidal
AB3E
VSPER code
Bent
AB3E2
VSPER code
Trigonal Bipyramidal
AB5
VSPER code
Octahedral
AB6
Structural formula
Electronegativity Chart
0 > .3 = nonpolar covalent
.4 - 1.8 = polar covalent
> 1.9 = ionic
Exception to the octet rule
Hydrogen- only 2 electrons.
Boron- 3 electrons.
Phosphorous/Sulfur- combine with fluorine, oxygen, and chlorine
Ionic bond
Electrical attraction of cations and anions
Ionic bond
Electrical attraction of cations and anions
Covalent bond
Sharing of electron pair between two atoms