Final Flashcards
What best describes how an immunoassay interacts in a blood serum
It recognizes the 3D shape of a specific molecule
When electrons are shared between two atoms outer electron shells, what kind of bond forms
a covalent bond
How does the formation of a covalent bond occur?
by the overlap of two atoms electron orbitals
When a compound forms because an electron or electron is transferred from one element to another, it is referred to as what type of compound?
ionic
Briefly describe the term valance electron
a single electron (or one electron out of a pair) in the outer shell of an atom that is responsible for the chemical properties of the atom
how does the Lewis Theory explain the loss or gain of electrons in an ionic bond?
atoms are attempting to achieve a stable noble gas or “octet” electron configuration
What do the valance shells of all the noble gas elements have in common
all have 8 electrons
As you move from the top to the bottom of the periodic table, what happens to the electronegativity of the elements
it decreases
How is the Br-H bond categorized?
polar covalent bond
Non polar covalent bonds
-occurs when the electronegativity of both atoms is equal
polar covalent bonds
-occurs when the difference in electronegativity is between .4 and 1.9
What is the electronegativity difference between the C-O bond? (C- 2.5, O- 3.5)
1.0
Many organic compounds have numerous C-H bonds. What is the average difference in electronegativity in one of them? (C- 2.5 ,H- 2.1)
0.4
How many bonds does carbon normally form?
4
How is ethane best represented by a lewis structure?
2 carbons that are bonded (C-C) with 3 bonds attached to each carbon
What is the formula for an alkane with ten carbons, decane
C10H22
Propane C3H8 is best represented by which lewis structure?
2 zig zag lines
Draw lweis structure for ethene C2H2 (a.k.a ethylene). How many double bonds does it have?
1
How many bonds does each carbon atom in an alkene normally have?
2 (double-bonded carbon and 2 single bonded elements)
meth-
1 carbon
eth-
2 carbons
prop-
3 carbons
but-
4 carbons
pent-
5 carbons
hex-
6 carbons
hept-
7 carbons
oct-
8 carbons
non-
9 carbons
dec-
10 carbons
alkanes
single bond
alkenes
double bonded carbon
alkynes
triple bonded carbon
How many carbon atoms should be in the molecule pentyne
5
How many carbon atoms should be in the molecule octanol
8
Ketone
R-(O=C)-R
Ketone end in
-one
alkanes end in
-ane
alkenes end in
-ene
alkynes end in
-yne
cycloalkanes
make rings (all elements are bonded to each other like a circle) (each point is a carbon)
cycloalkanes begin with
cyclo (wit prefix (meth, but, eth) before the cyclo)
ether
R-O-R
ether compounds end in
oxy
Esters
R-O-(C=O)-R
esters end in
-yl
alcohol
R-OH
alcohols end in
-ol
aldehyde
R-(C=O)-H
aldehydes end in
-al
carboxylic acid
R-(C=O)-OH
carboxylic acid end in
-oic acid
A double bonded alcohol compound with 4 carbons is called
methenol
COCl2 is an example of what type of electron-domain
tetrahedral
PF3 is an example of what type of electron-domian
trigonal pyramidal (<109.5)
a tetrahedral is bent at what angle
109.5
linear angle
180
Trigonal planar angle
120
SO3 is an example of what type of electron-domian
Trigonal planar
Solid
definite shape and definite volume, not compressible
Liquids
have no definite shape but do have a definite volume, able to flow
Gases
have no definite shape or volume. molecules very far apart (highly compressible)
Mixture
blending two or more “pure substances with variable composition
Pure substance
the components cannot be separated by any physical means (distilation etc.)
Elements
the simplest type of substance with unique physical and chemical properties. Consists of only one type of atom and cannot be broken down into simpler substances by any means (physical or chemical)
Compounds
structures that consist of two or more atoms that are chemically bound together and thus behave as an independent unit (ex. CO2)
Homogeneous Mixture
has the same properties and composition throughout the sample (ie. Salt water or brine is an aqueous homogeneous)
Heterogeneous Mixture
consists of two or more phases of variable composition that differ in properties (ie. water floating in oil)
Who created the periodic table
Dmitri Mendeleev
What are the three element classification
Metals, Nonmetals and metalloids
Metals Physical properties
- conduct heat/electricity
-solid (often hard except Hg)
-Metallic luster or shine
-Malleability (sheets) and ductility (wires)
Metals chemical properties
-released electrons to form cations
Nonmetals physical properties
-often gases (Br is a liquid)
- do not conduct
-brittle solids, dull appearance
- S, I, C, P (solids)
Nonmetals Chemical properties
-react with metals
-gain electron to form anions
Metalloids physical properties
-solids
-semiconductors
- ie. Si can conduct electricity at hight temps
Metalloids chemical properties
-form a variety of ionic, electron-deficient compounds
Which of the following states of matter is generally considered the most ordered?
solids
Cu
Copper
Ag
Silver
Au
Gold
Fe
Iron
chemical properties
substance’s potential to react with some other substances in its environment (ie. flammability, corrosiveness etc.)
Physical properties
properties measured without changing the chemical composition of the substance (ie. boiling point, freezing point)
Chemical changes
matter undergoes chemical changes to produce new substances
Types of chemical changes
-iron rusting
-burning wood
-metabolism
-cooking an egg
-baking a cake
-electroplating
-rotting banana
-vinegar and baking soda solution
-fireworks
-chemical battery
physical changes
changes of a substance between different forms of matter
Physical changes examples
-crushing a can
-melting an ice cube
-boiling water
-mixing sand and water
-breaking glass
-dissolving sugar in water
-shredding paper
-chopping wood
-mixing green and red marbles
-sublimation of dry ice
denisty =
mass / volume
density
ratio of an objects mass to its volume
atomic theory
-all matter is made up of tiny, invisible particles called atoms
-atoms cannot be created, destroyed, or transformed into other atoms in a chemical reaction
-all atoms of a given element are identical
-atoms combine in simple, whole-number ratios to form compounds
the law of multiple proportions
any time two or more elements combine in different ration, different compounds are formed
what is Ernest rutherford known for
the gold foil experiment
what are the three subatomic particles
electrons, neurons and protons
what are the 4 orbitals
s, p, d, f
Which orbital has the most energy
f
Which orbital has the least energy
s
s orbitals are (blank) shaped
spherically
p orbitals are (blank) shaped
dumbell
Group 1 (column 1) is what group
alkali metals
Group 2 (column 2) is what group
alkaline earth metals
group 17 (column 17) is what group
halogens
group 18 (column 18) is what group
noble gas
covalent bond
2 non metals
ionic bonds
have 1 metal and 1 nonmetal
valance bond theory
predicts that two nonmetals atoms will share electron in a covalent bond when there atomic orbitals overlap
