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Chem 103 > Unit one > Flashcards

Unit one Flashcards

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1
Q

What is the difference between a law and theory

A

a law describes an observation while a theory explains an observation

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2
Q

what questions do law and theories answer

A

laws answer what happened while theories answer why or how

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3
Q

what is the law of conservation

A

mass is neither created or destroyed

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4
Q

what is the law of definite proportions and what is another name for it

A

a substance is always made of the same proportions of elements; law of constant composition

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5
Q

what is the law of multiple proportions

A

elements combine in small, whole number ratios

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6
Q

what is Dalton’s atomic theory

A

matter is made of small, indivisible particles; atoms of a particular elements are identical; atoms of differnet elements are different; atoms combine in small, whole number ratios; atoms are neither created or destroyed

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7
Q

What is the mass defect effect

A

energy is lost due to the effort it takes to smoosh protons into nucleus thus the atomic weight of an atom is less than expected

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8
Q

what is the atomic number and how is it found

A

number of protons in an element; found on the periodic table

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9
Q

what is the mass number and how is it found

A

protons plus neutrons, found by calculation

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10
Q

what is an isoptope

A

atoms of the same element with different number of neutrons

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11
Q

what are ions

A

atoms that are not neutral due to different number of protons and electrons

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12
Q

what is the atomic mass

A

weighted average based on natural abundance of isotopes

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13
Q

what is the molecular formula

A

exact number of atoms in molecules

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14
Q

what is the empirical formula

A

ratio of atoms in a molecule

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15
Q

what is the symbol for wavelength and what does it mean

A

λ meaning the distance between any given point and the same point in the next wave

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16
Q

what is amplitude

A

the intensity of the waves

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17
Q

what is the symbol for frequency and what does it mean

A

v; how often there are waves per second

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18
Q

energy is _____ to v

A

proportional

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19
Q

energy is _____ to λ

A

inversely proportional

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20
Q

λ and v are _____

A

inversely proportional

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21
Q

how does energy leave an object

A

as light (in wavelengths)

22
Q

how does matter differ from gasses in terms of light

A

matter can exist at all stages of the visible spectrum but gasses can only exist at certain stages

23
Q

what is work function and its symbol

A

the E of a photon necessary to remove electrons from metal; Φ

24
Q

what happens when an electron drop an energy level

A

a photon is emitted by the atom

25
Q

what is the uncertaintly principle

A

it is impossible to simultaenously know the exact position and momnetum of a microscopic particle

26
Q

what is an atomic orbital

A

where electrons are likely to be found for each quantum state

27
Q

What is the principle quantum number, what does it describe, and what can it be

A

n; describes shells and the distance of electrons from the nucleus; anywhere from 1 to infinity

28
Q

what is the angular momentum quantum number symbol, what is its significance, what can it be, and what is its relationship with n

A

l; describes an orbital’s shape; and can be 0-3 or spdf; will always be less than n

29
Q

what are nodes

A

areas where electrons will never be found

30
Q

how do you find tha number of nodes in a subshell

A

n-1

31
Q

how do you find the number of angular or planar nodes in a subshell

A

l

32
Q

how do you find the number of radial or speherical nodes in a subshell

A

n-l-1

33
Q

what is the magnetic quantum number, what does it describe, and what can it be

A

m sub l; describes the number of orbitals in each subshell; can be 1,3,5 or 7

34
Q

what is the pauli exclusion principle

A

no 2 electrons in one atom may have any identical set of quantum numbers (electrons have to be different to be in the same subshell

35
Q

What is the aufbau principle

A

electrons in a ground state atom occupy the lowest energy orbitals available to them

36
Q

what is shielding

A

Happens when there are multiple electrons in an atom where they will be attracted to the nucleus but repeled from each other causing them to have much lower charge than expected and be held onto less resulting in them having higher energy

37
Q

What is the trend for shielding

A

Increases as you go right and down

38
Q

How does shielding affect orbitals

A

It causes lower orbitals to be more stable than higher ones

39
Q

what is the first l block anomaly

A

it is more stable for d orbitals to be half or fully filled so electrons will be taken away from s orbitals to fulfill this

40
Q

what does it mean for fluorine to be isoelectronic to helium

A

that when fluorine gains an electron it has the same electron configuration as helium

41
Q

what is the second l block anomaly

A

when losing electrons, d block elements will lose s electrons before losing d ones

42
Q

What is the effective molecular charge (Z effective) trend

A

as n and Z increases, Z effective increases

43
Q

what is Z effective

A

the net positive charge that an electron feels

44
Q

What do periodic trends depend on and how do they increase

A

Z and n; n increases down the periodic table while Z increases across the period table

45
Q

what is the atomic radius trend

A

as n increases, radius increases and as Z increases, radius decreases

46
Q

What is the ion radius trend

A

As Z effective increases, ion radius decreases (cations get smaller as they get more positive while anions get larger as they get more negative)

47
Q

What is ionization energy

A

The E required to completly remove an electron from an atom

48
Q

what is the Ionization energy trend

A

as n increases, IE decreases and as Z increases, IE increases

49
Q

How are ionization energy and atomic radius related

A

as atomic radius decreases ionization energy increases

50
Q

What is electron affinity

A

E releases when an electron is added to an atom

51
Q

What is the electron affinity trend

A

As Z increases, EA increases and as n increases, EA decreases

Chem 103 (5 decks)

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