Chemistry Test chapter 9 cumulative Flashcards
Name the type of bond that results from sharing of four electrons.
Double bond
Covalent bond
Know the equation for ideal gas law.
PV=nRT
What is the heat required to cause a unit rise in the temperature of a unit mass of a given substance?
Specific heat
Absolute zero equals …
-273.15 degrees Celsius
0 kelvins
What causes the bright colored lines in the spectrum of glowing hydrogen gas?
Each line is a photon emitted when an electron drops to a lower energy level
What property is used to predict whether a bond is primarily ionic or primarily covalent?
Electronegativity
Name the principle that states elements tend to react chemically to achieve a noble gas electron configuration whether by losing, gaining, or sharing electrons.
Octet rule
Know and understand Exothermic chemical reactions.
- chemical reaction releasing energy, usually causes the products to become hotter than the reactants because some energy was released.
Understand the differences between compounds and mixtures.
Compound- are combined in definite proportions , are chemically combined, lose their properties to form a new substance with new properties, can be separated only by chemical means
Mixtures- are present in variable proportions, are not chemically combined, each component retains its properties, can be separated by physical means
Name the covalent bond in which the bonding electron pair is pulled closer to the more electronegative element.
Polar bond
Understand the uncertainty principle.
- it is impossible to simultaneously determine the momentum and the position of an electron with precision; either momentum or position may be measured precisely but not both.
Know and understand covalent bond.
Sharing of one or more electron pairs between two atoms
- atoms of non metals of similar Electronegativity
Know and understand ionic bond.
Electrostatic force of attraction between ions resulting from transfer of electrons
- atoms of metals and non metals having widely different electronegativites
Know and understand metallic bond.
Delocalized electron cloud around metal atoms
- atoms of metallic elements
True/false
The second law of thermodynamics states that enthalpy of the universe is always increasing.
False
Entropy (disorder)
True/false
The simplest repeating unit in a crystal is a unit cell.
True
True/false
The molecule of CO2 in which two polar bonds point symmetrically in opposite directions is polar.
False
Nonpolar
True/false
Kinetic energy is associated with an object’s position.
False
Potential energy
True/false
The speed of light in a vacuum is approximately 3.00 x 10 (8) m/s.
True
True/false
Atoms that are of the same element but differ in the number of particles in the nucleus are isotopes.
That differ in mass numbers
True
True/false
A solid whose particles are characterized by a regular, repeating, three dimensional pattern is an amorphous solid.
False
Crystalline solid
Know formula for sodium sulfate.
Na2SO4
Name the type of chemical formula that is the simplest ratio of atoms in a compound.
Empirical formula
Formula unit- called this when referring to ionic compounds
What is PCI (5) - check test question number 30.
Phosphorous pentachloride
What particle that composes an atom has a negative charge?
Electron
Name the term that refers to a bonding situation in which electrons are shared by more that two atoms.
Delocalization
How long is 2.54 cm in millimeters.
.254 milli meters
Elements fluorine, brownie, and iodine are part of what category?
Halogens
Elements like magnesium, calcium and barium are part of what category?
Alkaline Earth Metals
What type of geometry does acetone in which three bonding pairs of electrons are arrayed around the central atom have?
Trigonal planar
Which of the following elements would you expect to have the greatest electro negativity ? Is it S, Ca, CI and/or Cs.
Cl
A +BC= AC+B
What kind of reaction?
Single displacement
What type of geometry does hydrogen selenide which has two bonding pairs and two no binding pairs of electrons around the central atom have?
Angular
Why does H2O have a higher boiling point than H2S?
Because oxygen has a higher Electronegativity causing its atoms to attract stronger than sulfur
Elements boron, silicon and geranium are part of what category?
Semi metals
Going from solid to liquid is what process?
Heat of fusion
Melting
Know and understand dipole-dipole force.
Found only in polar molecules
Fairly strong
Constant attraction between weak partial charges
Know and understand hydrogen bond.
Found only in molecules containing hydrogen covalently bonded to highly electronegative atoms
Very strong force
Constant attraction between relatively strong partial charges
Know and understand London force.
Found in all molecules
Very weak force
Momentary attraction between weak partial charges
The —— cubic arrangement of atoms in a crystal has the least empty space of any cubic arrangement.
Hexagonal close packing
The ——– law of thermodynamics relates change in internal energy to heat and work.
First
The outermost electrons in an atom which are involved in chemical bonding are called ——- electrons.
Valence
The ——- theory of light states that light is electromagnetic waves traveling as bundles or packets of energy.
Quantum
The mass of a substance per unit of volume is called ——.
Liters per mol
A theoretical gas that exactly obeys the assumptions of the kinetic theory would be called a(n) ——— gas.
Ideal
Know how to balance equations.
Good
Know how to draw the Lewis structure of phosphorus trichloride.
. . . . . .
:Cl— P —Cl:
. . \ . .
:Cl:
. .Using the periodic table, calculate the molar mass of benzene.
C6H6
See question 59.
Q
A sample of helium gas has a volume of 620. mL at a temperature of 500. K. If we decrease the temperature to 100. K while keeping the pressure constant what will the new volume be?
P•V P•V
—- = —-
T T
Hard substances like diamonds, silicon carbide and Quartz that contain covalent bonds but do not consist of discrete molecules are referred to as …
Crystalline solids- atoms or molecules regularly arranged
