Week 1 csv

Question 1

what is the difference between organic and inorganic chemistry

Answer 1

organic chemistry is the chemistry of carbon, its reactivity and relationships with other elements and the compounds carbon makes. can be further divided into: biological, ex:skin and non-biological, ex: plastic.
Inorganic chemistry is the chemistry of elements, reactivity and atomic relationships that are based on elements and their properties.

Question 2

atom

Answer 2

a single nucleus made of protons and neutrons, with a cloud of orbiting electrons

Question 3

what determines what the element of an atom is

Answer 3

the number of protons

Question 4

protons and neutrons cling to each other in a sphere called:

Answer 4

the nucleus

Question 5

atomic particles are composed of:

Answer 5

sub-atomic particles. Therefore, atomic particles are divisble.

Question 6

what does it mean that hydrogen appears as: H^0

Answer 6

it means it is unadulterated; the proton and electron count add to a charge of zero. 1 proton = + 1, 1 electron = - 1. together they equal 0

Question 7

the chemical properties of an element are determined by:

Answer 7

the number of electrons. In an ideal atom the count of electrons to protons is equal, but the electron count can vary easily

Question 8

valence number

Answer 8

the characteristic number of electrons lost or gained from the electron cloud of the atom.

Question 9

how is a valence number measured

Answer 9

a positive valence (+) means less electrons than protons. A negative valence (-) means more electrons than protons

Question 10

how is a molecule formed

Answer 10

when 2 or more atoms interact and bind together by electron behaviors

Question 11

isotope

Answer 11

one element with varying neutron counts

Question 12

periodic table

Answer 12

a chart of all the elements found in nature and synthetic elements created in nuclear reactors. It shows the chemical similarity between vertical columns of elements. It is organized by valence state of elements

Question 13

electroneutrality

Answer 13

the valence electron count of a molecule = 0
ex: O has a -2 state and if it combines with 2 hydrogen at +1 states each, 1+1-2=0
therefore, 2 hydrogen at +1 balances 1 oxygen at -2 for electroneutrality.

Question 14

covalent bonds

Answer 14

electrons cooperate. electrons are shared freely from one electron cloud to another, bonding an atom to another atom. *almost all carbon compounds are covalently bonded

Question 15

ionic bonds

Answer 15

charge polarities in molecules create electronic attraction of +/- which link atoms by attraction to their opposite charge.

Question 16

weak bonds

Answer 16

form between atoms that have a much less definitive ability to keep a compound bound together. weak pull towards one another, and easily torn apart. One major weak bond is a hydrogen bond.

Question 17

polarity

Answer 17

NOT SYMMETRICAL. Ex: water. Stable, but has a net off-balanced charge; has a positively charged side, and a negatively charged side.

Question 18

non-polarity

Answer 18

SYMMETRICAL. Even, symmetrical distribution of atoms, neutral / balanced charge due to the balance of its structures.

Question 19

ion

Answer 19

signifies an atom that is dissolved in water and has either a positive or negative charge. Can be single element or compound

Question 20

difference between a molecule and macromolecule

Answer 20

molecule is usually two or more atoms that are bound together creating complexity. Macromolecules are huge numbers of molecules bonded together to form giant molecules.

Question 21

dissolution

Answer 21

when an ionic compound, like NaCl, dissolves in water, the sodium +1 state and the chlorine -1 state go into solution, and the salt crystal is broken up, and the atoms are distributed throughout the water, but still electrically neutral.

Question 22

dissolution potential

Answer 22

determines how easily or how much of the compound will dissolve in water

Question 23

covalent molecules and dissociation:

Answer 23

covalent molecules also dissolve in water, but do not dissociate. Their asymmetrical charge distribution allows the polarity of water to put the molecule into solution

Question 24

solubility of polar and non-polar substances

Answer 24

polar substances dissolve in polar fluid like water. Non-polar substances will dissolve in non-polar fluids like carbon tetrachloride or oils

Question 25

cations vs. anions

Answer 25

cations equal positively charged ions like Na+ or Ca+2. anions equal negatively charged ions like Cl- or PO4-

Question 26

when anions and cations crystallize together, these dissolved ionic compounds are called

Answer 26

salts

Question 27

pH

Answer 27

percent hydrogen. scale of 1 - 14. 7 is neutral, (pure water); Acid strength increases as the rating goes to 1; bases increase in strength as the rating goes to 14. *when there is an excess of negative ions in a solution, the fluid will most likely be basic in nature.

Question 28

H+ is shorthand for:

Answer 28

hydronium

Question 29

what happens when an acid dissociates

Answer 29

the hydrogen ions H+ increase in number in the solution, which created an acid pH 1 - 7

Question 30

what is the most common anion that produces basic solutions

Answer 30

OH-. The more OH- that dissociates into water, the more powerful the base.