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yall mind if i move yalls test 2 wednesday? > CHAPTER 1 AND 2: FINALS REVIEW > Flashcards

CHAPTER 1 AND 2: FINALS REVIEW Flashcards

1
Q

from oldest to newest, list the different atomic models

A

Democritus’ model, Dalton’s atomic model, Thompson’s atomic model (the plum pudding model), Rutherford atomic model, Rutherford-Bohr atomic model, the simplified atomic model

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2
Q

what principles did Dalton’s model consist of?

A
  • All matter is composed of atoms
  • all the atoms of one single element are identical
  • atoms of differing elements are different
  • atoms of different elements can combine in fixed proportions
  • nothing is lost nor gained during chemical reactions
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3
Q

What did Thompson discover using cathode rays?

A

Using cathode rays he deduced that cathode rays are negatively charged (the rays are attracted to the positive pole of an electrical field), contains particles (able to move a propeller, able to cast a shadow) meaning they emit electrons, a particle that can detatch itself from an atom.

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4
Q

what three types of radiation can radioactive substances give off to eachother?

A

alpha, beta, and gamma rays

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5
Q

What happened during the gold foil experiment? What did it help deduce?

A

Ernest Rutherford deduced that some alpha particles were deflected and some bounced back (small, dense, positively charged nucleus), and many passed through (an atom is mostly empty space)

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6
Q

What did the Rutherford-Bohr model improve on regarding the atmoc model?

A

Through finding out that electrons can move to a higher orbit when charged, the model was given orbits

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7
Q

True or False: The simplified atomic model is the only model with neutrons?

A

True (added by James Chadwick)

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8
Q

Why were neutrons added?

A

If neutrons didn’t exist, nuclei would explode when being all positive

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9
Q

when talking about atomic mass and atomic numbers, what does z and a represent

A

Z- atomic number

A- atomic mass

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10
Q

What differes different isotopes?

A

Different number of neutrons

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11
Q

what three types of isotopes are there?

A

Natural isotopes - found in nature
Artificial isotopes - manufactured by bombarding atoms with other atoms
Radioactive istopes - break down radiactively, releasing radiation

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12
Q

How do you calculate an element’s relative atomic mass?

A

((relative abundance of isotope 1 x atomic mass) + ( “ “+…)/100

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13
Q

What are the 8 groups of the periodic table? what are their characteristics?

A 
Group 1 (alkali metals): soft, light, highly reactive, paired with halogens to form salts, low melting points
Group 2 (alkaline earth metals): hard, malleable, grey, found with rocks or with halogens 
Group 3 (Boron group): loses 3 electrons 
Group 4 (Carbon group): loses or gains 4 electrons
Group 5(Nitrogen group): gains 3 electrons
Group 6(Oxygen group): gains 2 electrons 
Group 7(halogen group): toxic, corrosive, bactericidal, colourful, reacts with H to form acids 
Group 8 (Noble gases): Colourless, stable, emit light when electrified, found in their elemental states
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14
Q

Name all trends of the periodic table. how to they increase and decrease?

A

Atomic radius - bigger on the left, smaller on the right. Caused by higher numbers of protons being attracted to the electrons on the atom’s orbits
Ionization energy: energy required to steal a valence electron from an atom. less of this on the right, more on the left. Increases going up
Electronegativity: energy an atom has to remove a valence electron. less on the right, more on the left. Increases going up
Chemical reactivity: how vigourously and atom will recat with others. More reactive on the left, less on the right

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15
Q

What is Avogadro’s number

A

6.023 x 10 to the power of 23

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16
Q

What is molar mass?

A

mass of a mol from a given substance measured in g/mol

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17
Q

What is the formula for finding molar mass

A

M=m/n (m being mass in g, n being number of moles)

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18
Q

What is the formula for finding the number of particles?

A

n= # of particles/avogardro’s #

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19
Q

What is a molecule

A

prticle formed by the combination of two or more elements

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20
Q

What is a compund

A

Pure substance formed by the combination of two or more elements

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21
Q

What’s an ion?

A

Atoms thats have lost or gained electrons

22
Q

Polyatomic ions are ions made of several atoms. What are the most common ones?

A

Acetate, ammonium, ammonia, bicarbonate, carbonate, chlorate, chromate, hydroxide, nitrate, nitrite, phosphate, sulphate, sulphite

23
Q

What is the difference between ionic bonds and covalent bonds

A

Ioinic: Bond between metal and non-metal. A metal will transfer the electrons
Covalent: Bond between two non-metals. the atoms will share the electrons

24
Q

What are the diatomic elements?

A

Hydrogen, nitogen, flourine, oxygen, iodine, chlorine, bromine (Have no fear of ice cold beer)

25
Q

What are the prefixes for covalent bonds?

A 
1 Mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca
finish the last element with "ide", dont use mono for the first element if suffix is 1
26
Q

How do you name ionic bonds

A
  1. +ve ion first
    2.use ide for negative ion
    Mention number of valence electrons for transition metals (e.g., Iron (III) phosphate)
    **Use crossover rule to go from name to formula
27
Q

what is an aqueous solution?

A

a solution in which the solvent is water

28
Q

what is a solution

A

a homogenous mixture where components cannot be distinguished no matter what

29
Q

How can we find concentration in g/L

A

C= m/v (mass, volume)

30
Q

How can we find concentration in mol/L

A

C=n/v (mol, volume)

31
Q

How can we find concentration percentage in g/mL

A

C= m1/m2 x100%

32
Q

How can we find concentration percentage in mL/mL

A

C= v1/v2 x100%

33
Q

How can we find concentration in ppm?

A

Cppm= mg/kg

34
Q

How do we calculate dilution?

A

C1V1=C2V2

35
Q

What is an electrolytic solution?

A

Solution with electrolytes

36
Q

What is electrolytic dissociation? How does it differ from molecular dissociation?

A 
When electrolytes (substances that allow electricity to flow when sperated in a solution) seperate into cations and anions 
vs.
When nonelectrolytes seperate and dont produce ions and do not conduct electricity
37
Q

what does the conductivity of a solution depend on?

A

of ions, mobility, changes in direction

38
Q

What are the three types of electrolytes?

A

Acids, bases, salts

39
Q

What determines an acid

A

The presence of H+ at the beginning (exlcuding acetic acid, an organic acid)

40
Q

What determines a base?

A

The presence oh OH- (excluding ammonia due to how it transforms into ammonium and hydroxide when dissolved in water)

41
Q

how do you name an acid

A

hyrdro+nonmetal+ic acid

42
Q

how do you name a base

A

Metal hydroxide

43
Q

What determines a salt?

A

bonding of a metallic and nonmetallic ion excluding OH- and H+

44
Q

True or False: all salts are neutral

A

False. some salts are more acidic and others are more basic

45
Q

Name two alcohols

A 
Ethanol  C(2)H(5)OH-
Methanol CH(3)OH- 
false bases
46
Q

Looking at the pH scale, what signifies if something is neutral and acid or a base

A

Acid - below 7
neutral - 7
basic- above 7

47
Q

What does the pH scale being logarithmic mean?

A

difference of one unit between two substances = one substance is 10x more acidic or basic than the other

48
Q

what is pOH? what is a pH

A
  1. potential of hydroxide

2. potential of hydrodgen

49
Q

How do you calculate pH? how do you calculate pOH?

A 
pH = -log(H+)
pH+pOH = 14
50
Q

how do you determine the concentration of hydrogen? what about concentration of hydroxide?

A 
(H+) = 10(thpwr of -pH)
(H+)(OH-) = 1x10(thpwr of -14)

yall mind if i move yalls test 2 wednesday? (5 decks)

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