Unit 1 Flashcards

1
Q

AMU

A

Atomic Mass Units (u)
the measurement of mass for elements

1 = ABOUT a proton/neutron - don’t count on this

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2
Q

molar mass

A

the mass of an element - measured by g/mol

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3
Q

Groups on a Periodic Table

A

the columns

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4
Q

Periods

A

the horizontal rows

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5
Q

Group 1A/1

A

Alkali Metals

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6
Q

Groupe 2A/2

A

Alkaline Earth Metals

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7
Q

Group b/3-12

A

Transition Metals

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8
Q

Group 7A/17

A

Halogens

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9
Q

Group 8A/18

A

Noble Gases

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10
Q

How do you determine the element?

A

The number of protons

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11
Q

Isotopes

A

a different number of neutrons

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12
Q

mass spectometry

A

a graph which has the mass and abundance of a certain element

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13
Q

Average Molar Mass Calculation

A

{(amu x % composition) …+…+(amu x %composition)}

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14
Q

Mole

A

6.022 x 10^23

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15
Q

Combined Gas Law

A

PV = nRT

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16
Q

What does R stand for in the Gas Law?

A

0.0821 L atm / mol K

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17
Q

What is the Standard Temperature and Pressure (STP)

A

P = 1 atm
T = 273 K

(Moles = Volume / 22.4 L/mol)

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18
Q

Molarity (M)

A

the measurement of calculation

(moles)/(volume)

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19
Q

What is THAT Molarity equation

A

M1V1 = M2V2

20
Q

Empirical Formula

21
Q

Molecular Formula

A

the actual composition of an element

22
Q

What are electrons energy like?

A

they are QUANTIZED.

the farther they are from the nucleus, the higher their potential energy

23
Q

Electromagnetic Radiation

A

energy in the form of waves

24
Q

When an electron goes from a high energy level to a low energy level, it….

A

emits energy

25
Q

When an electron goes from a low energy level to a high energy level, it…

A

absorbs energy

26
Q

Ionization/Binding Energy

A

the energy level for an electron to be ejected

27
Q

Incoming Radiation Energy Equation

A

(Binding Energy) + (Kinetic Energy)

Kinetic Energy = ejects the electron

faster = more Energy

28
Q

What is the unit used for Ionization Energy?

28
Q

eV = ?

A
  1. 60 x 10^-19 Joules
29
Q

Photoelectron Spectra (PES)

A

the chart for binding energy and number of electrons

30
Q

n is equal to what?

A

energy level

31
Q

l is equal to what?

A

shape (n-1)

32
Q

Electron Configuration

A

the equation that tells you electron configuration

33
Q

What is the shorthand for electron configuration?

A

[Nobel Gas] + configuration

34
Q

Aufbau Principle

A

the electron is placed in increasing Energy subshells

35
Q

Pauli Excursion Principle

A

the electrons spin in OPPOSITE directions

36
Q

Hund’s Rule

A

electrons pair up only after they have filled up all their other subshells

37
Q

What is stability based on in an electron?

A

if the last orbital is filled

38
Q

What is a valence electron?

A

the electrons in the last energy level (!)

39
Q

Electronegativity

A

electron attraction of an element

40
Q

what is electronegativity have depended on and what is the trend?

A
  1. smaller radius = higher electronegativity
    down, decrease
  2. shell completion
    left to right increase
41
Q

Electron Affinity

A

change in energy that occurs when an electron is added to a neutral atom

generally exothermic reaction

42
Q

Effective Nuclear Charge (Zeff)

A

the positive attraction that the electron feels

43
Q

Electron Shielding

A

an inner electron blocks the electron on the outer layer - blocking attraction
lowering Zeff

44
Q

mass number

A

(number of protons) + (number of neutrons)

45
Q

What is the equation of Zeff for an electron

A

Zeff = Z - S

Z = atomic number
S = sheilding effect

46
Q

Binding Energy Equation

A

BE = hv - KE