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chapter 2 Flashcards

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1
Q

what is the atomic theory?

A

The theory that all matter is composed of atoms grew from observation and laws.
1. The Law of Conservation of Mass
2. The Law of Definite Proportions
3. The Law of Multiple Proportions

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2
Q

According to Dalton’s atomic theory, the hypothesis about the nature of matter can be summarized as follows:

A
  1. Elements are composed of extremely small particles called atoms.
  2. All atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements.
  3. Compounds are composed of atoms of more than one element. For any given compound, the atoms present are always in the same ratio.
  4. A chemical reaction involves only the separation, combination, or rearrangement of atoms: it does not result in the creation or destruction of atoms.
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3
Q

what is the law of conservation of mass?

A

The Law of Conservation of Mass: states that in a chemical reaction, matter is neither created nor destroyed

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4
Q

compare the mass of the reactants to the mass of the products according to the law of conservation of mass?

A

The mass of the reactants = the mass of the product
Particles rearrange during a chemical reaction, but the amount of matter is conserved, because the particles are indestructible (at least by chemical means).

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5
Q

what is the law of definite proportions?

A

states that all samples in a given compound, regardless of their source or how they are prepared, have the same proportions of their constituent (basic/integral) elements

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6
Q

what is an example of the law of definite proportions?

A

Example: Water (H2O) will always have 2 parts hydrogen to 1 part oxygen by mass, no matter how much water you have.

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7
Q

what is the law of multiple proportions?

A

states that when two or more elements combine in different ratios, different compounds are formed

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8
Q

what is john dalton’s atomic theory?

A
  1. Each element is composed of tiny, indestructible particles called atoms.
  2. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements.
  3. Atoms combine in simple, whole-number ratios to form compounds.
  4. Atoms of one element CANNOT change into atoms of another element.
    In a chemical reaction, atoms change the way that they are bound together with other atoms to form a new substance.
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9
Q

what are the correct and incorrect aspects of john dalton’s atomic theory?

A

Correct aspects:
- All matter is made up of tiny particles called atoms, and atoms of different elements have different properties.
Incorrect aspects:
- Atoms are not indivisible (they can be broken down into smaller particles like protons, neutrons, and electrons), and atoms of the same element can have slightly different masses due to isotopes.

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10
Q

what are atoms composed of?

A

Atoms are composed of even smaller, more fundamental particles including:
Electrons
Protons
Neutrons

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11
Q

what is the difference between an atom and an element?

A

An atom is the smallest unit of matter, consisting of protons, neutrons, and electrons, while an element is a pure substance made up of only one type of atom

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12
Q

what are electrons mass and charge?

A

Electrons has NO mass and has a NEGATIVE charge

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13
Q

what are protons mass and charge?

A

Protons have a mass and a POSITIVE charge

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14
Q

what are neutrons mass and charge?

A

Neutrons have a mass and NO charge

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15
Q

what are electrons’ and protons’ relationships in magnitude and charge?

A

Electrons and protons are EQUAL in magnitude but OPPOSITE in charge

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16
Q

what are protons and neutrons relationship in mass?

A

Protons and neutrons are EQUAL in mass

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17
Q

If we have two OPPOSTIELY charged particles, they will…..

A

If we have two OPPOSTIELY charged particles, they will ATTRACT

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18
Q

If we have two SIMILARLY charged particles, they will …

A

If we have two SIMILARLY charged particles, they will REPEL

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19
Q

If we have two particles that are equal in magnitude and but opposite in charge, they will…

A

If we have two particles that are equal in magnitude and but opposite in charge, they will cancel each other out. So two charged particles when they’re reacting - they have no net charge.

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20
Q

what is Coulombs law? what does it tell us about the relative attraction or repulsion?

A

We could determine the relative attraction or repulsion between two particles using Coulomb’s law: the attraction and repulsions between charged particles are described by Coulomb’s law, which states that the potential energy (E) of two charged particles depends on the charged (q1 and q2) and their separation (r).

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21
Q

what is the equation for coulombs law?

A

Which is: E = q1*q2/r

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22
Q

negative energy is related to which one (attraction/repulsion)?

A

When we talk about attraction (two particles being attracted to each other) we are referring to negative energy. (-)

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23
Q

positive energy is related to which one (attraction/repulsion)?

A

When we talk about repelling (two particles being repelled against each other) we are referring to positive energy. (+)

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24
Q

the magnitude of the attraction or reputation depends on what?

A

The magnitude of the attraction or repulsion depends on other characteristics - how close the particles are, etc.
- If two negative particles are really close to each other, there will be a really high repulsion energy - because the ‘r’ is really small, which is the separation.
- But if the particles are a little further apart, they are still not attracted to each other - but since the distance increased, the repulsion is a little less.

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25
Q

for like charges, what happens to the potential energy?

A

For like charges, the potential energy (E) is positive and decreases as the particles get farther apart (as r increases).

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26
Q

for opposite charges, what happens to the potential energy?

A

For opposite charges, the potential energy (E) is negative and becomes more negative as the particles get closer together (as r decreases).

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27
Q

The magnitude of the interactions between charged particles _______ as the charges of the particles increase.

A

The magnitude of the interactions between charged particles increases as the charges of the particles increase.

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28
Q

what did we learn about the cathode ray tube?

A

If the rays bend toward the positive plate, it concludes that the cathode rays are negatively charged.
If the rays bend towards the negative plate, it concludes that the cathode rays are positively charged.

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29
Q

what did we learn about the oil drop experiment?

A

The point of Milikan’s oil drop experiment was to find out the charge of an oil drop, or electron.

The formula is charge * mass/charge = mass
-1.60 10^-19 C * g/-1.7610^8 C = 9.10 *10^-28g

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30
Q

define radiactivity

A

Radioactivity is the spontaneous emission of high-energy radiation and particles by materials.

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31
Q

define alpha particles

A

Alpha (a) particles have a radioactive emission with a charge of 2+ and a mass equivalent to that of a helium nucleus.

32
Q

what was the plum pudding theory?

A

His theory was that negative particles must be suspended in a positive mass. And these positive masses must be equal in magnitude to the negative particles, but opposite in charge.

33
Q

what was put into place to test the plum pudding theory?

A

gold foil experiment to test the plum pudding theory.

34
Q

what did we learn from the gold foil experiment?

A

Results indicate the presence of dense particles WITHIN the atom, which proves one of the theories to be untrue ^^.
That led us to an idea of a more accurate representation of an atom, where the positive charge is concentrated in the center, and the negative electrons are around the nucleus.

35
Q

what is the atomic number?

A

The atomic number (Z) is written small in the left subscript (bottom), and it tells us the number of protons.

36
Q

What is the mass number?

A

The mass number (A) is written small in the left superscript (top) and it tells us the number of nucleons in an atom - which is the number of protons + the number of neutrons.

37
Q

how do you find the number of neutrons?

A

Mass number - number of protons = neutrons

38
Q

how do we find the number of electrons?

A

Because elements are neutral, if we know the number of protons, we know the number of electrons.
Protons = electrons in a neutral element

39
Q

what was the purpose of the positive-ray analyzer ?

A

This was done by Francis W. Aston and he developed this positive-ray analyzer which led to the discover of isotopes.

40
Q

define isotopes

A

Isotopes- are atoms of an element containing the same number of protons but different numbers of neutrons

41
Q

if isotopes of elements have different numbers of neutrons, what does this mean?

A

This means that since there is a different number of neutrons, there would be a different mass number

42
Q

define periodic law

A

Periodic law: when the elements are arranged in order of increasing mass, certain sets of properties recur periodically.

43
Q

what are main group elements?

A

aka representative elements, the elements in groups 1, 2, and 13-18 of the periodic table.
“A” elements

44
Q

what are transition metals?

A

Transition metals: the elements in groups 3-12 of the periodic table
“B” elements

45
Q

what are metals and where are they located?

A

Metals: are typically shiny solids that conduct heat and electricity well and are malleable and ductile.
To the left of semimetals

46
Q

what are nonmetals and where are they located?

A

Nonmetals: are elements with properties opposite those of metals including poor conductivity of heat and electricity
To the right of semimetals (but including hydrogen)

47
Q

is hydrogen a nonmetal or a metal?

A

Hydrogen is a nonmetal.
Depending on what hydrogen is binding to, it can act like a metal or a nonmetal.

48
Q

what are semimetals/metalloids?

A

They are elements along the border of the periodic table between metals and nonmetals; they have some metallic and some nonmetallic properties.
Everything to the left of semimetals is metal (except for H)
Everything to the right of semimetals is nonmetal

49
Q

what are periods?

A

Periods: are the horizontal rows in the periodic table

50
Q

what are groups?

A

Groups or families: are all elements in the same vertical column of the periodic table
They have similar chemical properties

51
Q

where are the noble gases and what are their characteristics?

A
  • Noble Gases: elements in group 18 of the periodic table.
  • Chemically unreactive
52
Q

where are the halogens and what are their characteristics?

A
  • Halogens are elements in group 17 of the periodic table
    The word halogen is derived from the Greek for “salt producer”.
  • Faiurly reactive nonmetals
53
Q

Where are the alkaline earth metals and what are their characteristics?

A

Alkaline Earth Metals: are elements in group 2 of the periodic table
- Form 1:2 compounds with all group 17 elements
- Form 1:1 compounds with group 16 elements
- Fairly reactive metals

54
Q

where are the alkali metals and what are their characteristics?

A
  • Alkali Metals: are elements in group 1 of the periodic table.
  • Form 1:1 compounds with all the group 17 elements
  • From 2:1 compounds with the group 16 elements
  • All reactive metals
55
Q

pure substances can either be ___ or ____

A

elements or compounds

56
Q

elements can either be ____ or _____

A

atomic or molecular

57
Q

what is an atomic element?

A
  • A single element - for example, Ne.
  • They are elements that exist in nature with single atoms as their basic units.
58
Q

what is a molecular element?

A
  • A pure substance made up of two or more atoms of the same element bonded together - for example, O2 (twins).
  • They are elements that exist as molecules, two or more atoms of the element are bonded together.
59
Q

what are two types of molecular elements?

A

Diatomic and polyatomic

60
Q

what are the diatomic molecules?

A

Br2, I2, N2, O2, Cl2, H2, F2

61
Q

what are the polyatomic molecules?

A

P4, S8, Se6

62
Q

compounds can either be _____ or ______

A

molecular or ionic

63
Q

what are molecular compounds?

A

composed of two or more nonmetal atoms that share electrons with one another in a covalent bond. For example, H2O

64
Q

what are ionic compounds?

A

any of a large group of chemical compounds consisting of oppositely charged ions, wherein electron transfer, or ionic bonding, holds the atoms together. For example: NaCl

65
Q

Atoms frequently gain or lose electrons. Why?

A

To gain stability.

66
Q

what are cations?

A
  • Cations are positively charged particles created when an atoms or molecule LOSES one or more electrons.
  • Cations are always smaller than their neutral counterpart.
  • Cations lose an electron, so they become smaller
  • Positive charge
67
Q

what are anions?

A
  • Anions are negatively charged particles created when an atom or molecule GAINS one or more electrons.
  • Anions gain an electron, so they become bigger.
  • Negative charge
68
Q

a metal tends to lose/gain electrons?

A

A metal tends to LOSE electrons, forming a CATION

69
Q

a nonmetal tends to lose/gain electrons?

A

A nonmetal tends to GAIN electrons, forming an ANION

70
Q

what are chemical bonds?

A
  • chemical bonds form because of the attraction between the charged particles (the electrons and protons) that compose atoms.
  • Compounds are composed of atoms held together by chemical bonds.
71
Q

what is bond energy?

A

the strength of the force between atoms (how much energy it takes to pull 2 things apart)

72
Q

what are ionic bonds?

A
  • they occur between metals and nonmetals.
  • they involve the transfer of electrons from one atom to another
73
Q

what are covalent bonds?

A
  • they occur between two or more nonmetals.
  • they Involve the sharing of electrons between two atoms
74
Q

Atoms held together by covalent bonds from ______ compounds

A

Atoms held together by covalent bonds from molecular compounds

75
Q

what are metallic bonds?

A

occur between metals and nonmetals

76
Q
A

Gen Chem I (2 decks)

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