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;
34 Cards in this Set
- Front
- Back
What bonds does oxygen and nitrogen havE?
|
nitrogen- triple
oxygen-double |
|
Are polar molecules asymmetrical or symmetrical?
|
asymmetrical
|
|
Is dipole polar or nonpolar molecule?
|
polar
|
|
Are non-polar molecules asymmetrical or symmetrical?
|
symmetrical
|
|
What are nonpolar molecules with polar bonds?
|
two different nonmetals that are asymmetrical
|
|
Why does metals conduct electricity?
|
because they have mobile electrons
|
|
How is metallic bonding sometimes described?
|
positive ions in a sea of electrons
|
|
Where do hydrogen bonds occur?
|
between H and elements that have high electronegativity and am small nucleus (N, F, O)
|
|
The high boiling point of water is due to
|
hydrogen bonds
|
|
When do Van der Waals forces become stronger?
|
when molecule size increases, and distance between them decreases
|
|
What part of an atom's structure seems to be largely responsible for its chemical properties?
|
outer orbit, electrons
|
|
What is ionic bonding?
|
transfer of one or more electrons from metals to nonmetals
|
|
What is covalent bonding?
|
two atoms share electrons instead of transferring them
|
|
When an ionic bond is formed between two atoms, each atom usually attains an outer shell arrangement similar to what group of elements?
|
Group 18
|
|
What is an ion?
|
an atom which has gained or lost one or more of its valence electrons
|
|
What is energy?
|
potential energy is stored in molecules and released in the form of chemical energy
|
|
When a chemical bond is formed, energy is
|
released
|
|
The more energy given off when a bond is formed
|
the more stable the bond is
General Rule: As energy is released, the stability of the system increases |
|
What is chemical bond?
|
simultaneous attraction of electrons to two or more nuclei
-electron may be transferred or shared either equally or unequally between two atoms |
|
Why do noble gases tend NOT to bond?
|
because they have 8 valence electrons
|
|
Ionic properties
|
-Ionic solids often form crystal structures held in fixed positions
-When melted or dissolved in water, the crystal structure is destroyed and the ions flow freely, this free movements allows for electrical conductivity |
|
What are molecular substances?
|
substances that contain covalent bonds are known as molecular substance and each particle is called a molecule
|
|
The greater the difference of electronegativity the (more, less) polar a bond is
|
more
HF- most out of other hydrogen bonds |
|
The element that has a higher electronegativity is
|
the negative pole
*Opposite: the element that has a lower electronegativity is the positve pole **known as dipole |
|
Metallic bonding occurs between atoms of metals
|
that have low ionization energies
|
|
Network solids (covalent)
|
-exception to softness
-examples: diamond, silicon dioxide, sand |
|
What substances have the highest melting/boiling point?
|
-metallic
-then ionic -covalent the least |
|
Is CO2 (carbon dioxide) polar in the intramolecular or the intermolecular?
|
Intramolecular- polar
Intermolecular- non-polar |
|
All diatomic particles are non polar for both
|
intermolecular and intramolecular
|
|
What physical properties are affected by intermolecular forces?
|
surface tension, solubility, melting and boiling points
|
|
What is a dipole?
|
-is the asymmetrical distribution of electrical charge in a molecule
-In a dipole, one end of the molecule is more negative than another |
|
The hydrogen bonding in water causes a (low/high) vapor pressure and (low/high) boiling point?
|
low vapor pressure
high boiling point |
|
Molecular-ion attractions are present in
|
aqueous solutions
|
|
Water molecules
|
are polar with polar covalent bonds
|