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Advanced Chemistry > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Mass

A

(g or kg) a measure of the amount of matter in an object, m=dv

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2
Q

Volume

A

(mL or cm^3) the space occupied by an object, v=m/d

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3
Q

Density

A

(g/mL or g/cm^3) amount of mass for every unit of volume, d=m/v

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4
Q

Metric Conversions

A 
Kilo=1000 units
Hecto= 100 units
Deka= 10 units
Base Unit
Deci= 0.1 units
Centi-= 0.01 units
Milli= 0.001 units
-King Henry Died By Drinking Chocolate Milk
-Use dimensional analysis
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5
Q

Significant Figure Calculations

A

Purpose: to show the precision of your measurement tool.
When adding/subtracting, round the answer to the number of decimal places of the least precise measurement (ex: 20.1cm + 10cm= answer with no decimal places b/c 10 is the least precise)
When multiplying/dividing, round your answer to match the amount of significant figures in the least precise measurement (ex: 220.000g / 2mL= answer with 1 sig fig b/c 2 is the least precise measurement and has 1 sig fig)

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6
Q

Scientific Notation

A

a way to shorten very large and very small numbers to make them easier to work with.

ex: 2,500,000= 2.5 x 10^6
- move the decimal place to the space just before the last number furthest from the decimal.

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7
Q

Mole Conversions

A

One mole of anything is 6.022 x 10^23 particles
To perform Mole conversions use dimensional analysis:
ex:
How many molecules of water are in 6 mol?
(6mol / 1)(6.022x10^23 / 1mol) = 4 moles
How many moles is 8.74x10^23 atoms of platinum?
(8.74atoms / 1)(1mol / 6.022x10^23 atoms)= 1 mole

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8
Q

Democritus

A
  • First person to propose that matter is composed of atoms
  • atom model looked like a ball
  • “Thought experiement”: if you took a material and kept dividing it in half, you should eventually reach a limit at the smallest particle, the atom
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9
Q

Dalton

A
  • revived the idea that matter is composed of atoms, based on experimentation with gases
  • atom model looked like a ball
  • findings led him to propose the Law of Conservation of Mass
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10
Q

Crookes

A

-discovered the electron using Cathode ray experiments

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11
Q

Thomson

A
  • experimented with a Cathode ray, showed that all atoms contain negative particles (electrons) along with Crookes
  • put together the “plum pudding’ model, a ball with positive and negative particles scattered throughout it
  • determined relative mass
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12
Q

Rutherford

A
  • Gold foil experiments; shot alpha particles through the foil
  • discovered the nucleus
  • atom model has a nucleus in the center with electron particles around it, electron arrangement did not make sense because it portrayed an unstable atom
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13
Q

Bohr

A
  • modified the Rutherford model
  • model include electrons in orbitals, each orbital containing a certain number of electrons to create a stable atom
  • discovered that electrons mo`ve in orbits around nucleus
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14
Q

Schrodinger

A
  • made most accurate atom model today

- model features electron clouds surrounding a nucleus

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15
Q

Atomic Number

A
  • equal to the amount of protons in an element
  • identity of element
  • 1/2 of the atomic mass
  • located above each element symbol on the PT
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16
Q

Atomic Mass vs Mass Number

A

Atomic mass:
-also known as atomic weight
-the weighted average mass of an atom of an element based on the relative natural abundance of that element’s isotopes.
Mass number:
-total number of protons + neutrons in a given isotope of an atom

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17
Q

Relative Abundance of Isotopes

A

(mass of isotope x decimal form of abundance) + (mass of isotope x decimal form of abundance) + etc- add masses of each isotope together

18
Q

Isotopic Notation

A

-At element symbol is featured big in the center
-Atomic Mass goes in the top left corner
-Atomic Number goes in the bottom left corner, technically unnecessary when given the symbol
-sometimes the charge is put in the top right corner
*Hyphenated isotope notation:
name of element- mass number of isotope
ex: Oxygen-16

19
Q

Ions

A
  • Atoms that have gained or lost electrons to become more stable
  • To find an ion’s charge, add the electrons and protons together, incorporating their relative charges
20
Q

Wave-particle duality of electrons and light

A

wave:
-Elements emit only specific colors of light when heated
-light is a form of electromagnetic radiation
-the longer the wavelength, the lower the frequency
The particle nature of light:
-quantum concept is the theory that matter can gain and lose energy only in small, specific amounts called quanta
-> concept developed by Max Planck- relates colors given off by elements to locations of electrons in discrete energy levels

21
Q

3 properties of electromagnetic radiation

A

1) Wavelength
2) Frequency
3) Amplitude

22
Q

Light Equations

A

As a wave: speed of light(c) = wavelength(lambda) x frequency(v)
As a particle: energy of one photon(E) = planck’s constant(h) x frequency(v)

23
Q

A laser emits light of frequency 4.74 x 10^14 sec^-1. What is the wavelength of the light in nm? (1m = 1 x 10^9nm)

A

633 nm

24
Q

A photon of light has a frequency of 1.50x10^14 Hz. Determine the wavelength and energy of the photon. Respect significant figures and write your answer in scientific notation.

A

wavelength: 2.00x10^-6 meters(m)

energy of the photon: 9.94x10^-20 joules(J)

25
Q

Calculate the wavelength of a photon of light with a frequency of 6.5 x 10^14 Hz.

A

4.6 x 10^-7 m

26
Q

Electromagnetic spectrum general trends

A

Visible Light should exist roughly in these parameters: wavelength= 300 - 800nm
frequency= something x 10^14s^-1
Energy of a photon= something x 10^-19 J/photon

27
Q

Bohr’s model of the atom

A
  • first model of the electron structure
  • gives levels where an electron is most likely to be found
  • incorrect today, but key in understanding the atom
  • In order to determine ENERGY LEVELS (n), Bohr used energy transfer on hydrogen atoms
  • Energy from an electron is released when electron falls inward, to an energy level closer to the nucleus emitting the energy (often as light)
  • Energy is added to an electron when electron moves upward, to an outer energy level (absorbs energy)
  • 1st shell=2 electrons
  • 2nd shell=8 electrons
  • 3rd shell=18 electrons
28
Q

Max number of electrons at an energy level

A

energy level 1 - 2 electrons
energy level 2 - 8 electrons
energy level 3 - 18 electrons
energy level 4 - 32 electrons

  • 1st quantum number (n)
  • 2n^2 is the formula to find it
29
Q

Orbital shapes, names, numbers

A
  • 2nd quantum number (l), will always be one less than 1st quantum number (n)
  • Shape of s sublevel: ball shape, l=0
  • Shape of p sublevel: dumbbell shape, l=1
  • Shape of d sublevel: clover shape, l=2
  • Shape of f sublevel: weird shape, l=3
30
Q

Electron configuration

A

-Shows the order in which electrons build up around the nucleus

31
Q

write electron configuration for Sodium, Boron, Oxygen, and Bromine

A

Sodium: 1s^2 2s^2 2p^6 3s^1
Boron: 1s^2 2s^2 2p^1
Oxygen: 1s^2 2s^2 2p^4
Bromine: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5

32
Q

How many electrons does each orbital within a shell hold?

A

2 electrons

33
Q

Noble gas shortcut

A
  • only show the electron configuration after the last noble gas (aka valence electrons)
  • write preceding noble gas in brackets, then start at the energy level below the noble gas and continue normal
34
Q

What is the electron configuration of Tellurium (using the Noble Gas shortcut)

A

[Kr} 5s^2 4d^10 5p^4

35
Q

Valence electrons

A
  • electrons that reside in the outermost shell surrounding an atomic nucleus
  • found in the orbitals associated with an atom’s highest occupied energy level
    - ex: [Kr] 5s^2 4d^10 5p^4, 5 is highest energy level-> add number of electrons tied to energy level 5-> 2 + 4 = 6 valance electrons
36
Q

Orbital Notation

A

Practice here: https://quizizz.com/admin/quiz/5dc18e821961d7001bace424/orbital-notation-practice

What is the orbital notation for Oxygen? Determine the 4 quantum numbers (n, l, ml, ms) as well using the orbital notation.

What is the orbital notation for Iron? Determine the 4 quantum numbers as well using the orbital notation.

37
Q

Pauli exclusion principle

A

no 2 electrons will ever have the same quantum numbers or share a room (spin state in an orbital)
-In orbital notation there will never be two side-by-side up arrows or two side-by-side down arrows in the same orbital

38
Q

Aufbau principle

A

lower energy sublevels fill up before higher energy sublevels
-electrons will always seek the lowest energy level (unless excited by a large input of energy like heat)

39
Q

Hund’s rule

A

electrons occupy their own orbitals before pairing up

-In orbital notation up arrows in each orbital fill up first and pair with down arrows after, if needed

40
Q

Avogadro’s Number

A

6.022x10^23 things/mole

41
Q

Speed of Light

A

3.00x10^8 m/s

42
Q

Planck’s Constant

A

6.626x10^-34 Js

Advanced Chemistry (1 decks)

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