Chemistry Midterm

Front 1

1 km

Back 1

1000 m

Front 2

1 m

Back 2

10 dm

Front 3

1 m

Back 3

100 cm

Front 4

1 m

Back 4

1000 mm

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1 m

Back 5

1 x 10 micrometers (um)

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1 m

Back 6

1 x 10 nanometers (nm)

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1 m

Back 7

1 x to picometers (pm)

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1 L

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1000 mL 1000 cm 1 dm

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K

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C = 273

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C

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K-273

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Energy

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1 cal = 4.184 Joule (J)

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D=

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M/V

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V=

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M/D

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M=

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D X V

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Speed=

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dist/time

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Time=

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dist/speed

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Distance=

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speed x time

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E=

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hf

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Frequency=

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speed of light / wavelength

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Speed of light=

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3.00 x 10 m/s

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Wavelength=

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speed of light / frequency

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1 hour=

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60 minutes

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1 min=

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60 seconds

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1 hour=

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3600 seconds

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Atomic number

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gives us the number of protons in the nucleus (the number of protons identify the element)

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number of neutrons=

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mass number - atomic number

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The atomic number doesnt give you both the protons and electrons, it officialy gives you the number of protons and you assume its the number of electrons

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true

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mass number

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total number of protons and neutrons in the atom (atomic mass rounded)

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chemical symbol

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is a shorter way of writing an element. the mass is on the left top corner and the atomic number is on the bottom left corner.

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why arent the masses on the periodic table for each element whole numbers?

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scientists take into account the 5 abundance when calculating the average atomic mass

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how do you calculate the isotope?

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1. move decimal 2 places to left to get rid of the 5
2. multiply answers from 3 1 by mass of the appropriate isotope
3. add your answer from step 2
4. write answer in amu (atomic mass unit)
This is known as the weighted atomic mass)

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isotopes

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atoms of an element with different numbers of neutrons (these will have different masses)

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what is the mass of a proton

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1 amu

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what is the mass of a neutron

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1 amu

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what is the mass of a electron

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0 amu (1/1840 amu)

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atomic mass unit

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1/12 the mass of a carbon atom

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The Bohr Model

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How the energy of an atom changes when it absorbs or emits light. An electron is found only in specific circular paths, or orbitas, around the nucleus. The farthe away from the nucleus, the closer together the energy levels are to one another. Amount of energy in a quantum can change. Electrons dont want to stay in the exciting state (they want to jump back to the ground state and release the same packet of energy int he form of light) Electrons are alsways moving and need to be supplied with energy.

Front 38

The Quantum Mechanical Atom

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modern description of the electrons in an atom.It determines the allowed energies an electron can have and how likely it is to find the electron in various locations aroudn the nucleus

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maxiumum number of electrons in energy level 1

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2

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maxiumum number of electrons in energy level 2

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8

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maxiumum number of electrons in energy level 3

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18

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maxiumum number of electrons in energy level 4

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32

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principle quantum number

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designates energy level (or section)

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sublevel (row)

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within the section of the energy level but ina different position

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sublevel s

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2 electrons, 1 oribital, sphere

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sublevel p

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6 electrons, 3 orbitals, dumbell

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sublevel d

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10 electrons, 5 orbitals, clover

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sublevel f

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14 electrons, 7 orbitals, funky

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electron configuration

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shorthand configuration to show where the electrons are

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what does the arrangment of electrons determines?

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the chemical properties of an element

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if you add up the superscripts in an electron configuration you get what?

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number of electrons

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after the 1 sublevel is full, why do electrons then fill the 2 s sublevel instead of the 2 p?

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electrosn always want to be on the least energy level closest to the nucleus ("ground state")

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shortcuts for electron configuration

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use the noble gasses from the previous period and write the electron configuration

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Aufbau Principle

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electrongs occupy orbitals of lowest levels. orbital filling diagrams.

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Paul exclusion principle

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electrons have to have opposite spin

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unshared electrons

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you do the orbital filling diagrams and whichever isnt complete is one unshared electron

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highest energy level

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add the superscripts of all the highest energy level numbers

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Hunds Rule

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the elecrons are going to occupy the orbitals singly before pairing up

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exceptions to electron configurations

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Cr and Cu

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what does light consist of?

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waves

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what does each wave cycle start at

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0

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amplitude of a wave

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waves height from zero the crest

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wavelength

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the distance bewteen the crests

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frequency

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number of wave cycles to pass a given point per unit of time (hertz)

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electromagnetic radiation or spectrum radiation

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radio waves, microwaves, infared waves, visible light, ultraviolet waves, x rays and gamma rays. all of hten travel ina vaccuum at a speed of light. light energy that comes from the sun.

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different frequencies seperate into a what

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spectrum of colors

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atomic emission spectrum

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whent the light passes through the prism, the frequencies of light emitted by an element separate into discrete lines to give the atomic emisison spectrum of the element

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continuous spectrum

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rainbow pattern that appears when white light is seperated

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spectroscope

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instrument used to separate light

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atomic emission spectrum or line spectrum

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looks like a bar caode (like the fingerprints of an element)

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Doberrine

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traids of elements whith similar properties

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Mendeleev

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arranged elements in groups with similar properties and ordered elements by increasing atomic mass

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Moseley

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arranged elements by atomic number instead of mass (how it is now)

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periodic law

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with elements arranged by increasing atonic number, there is a repeating pattern in the physical and chemical properties

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metals

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solid, good conductors of heat, ductile, malleable, other than mercury (solid at room temp)

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nonmetals

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most gasses, brittle, not good conductors of heat. S and P are solids and Br is a liquid

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metalloids

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have properties of both metals and nonmetals

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group 1

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alkali metals

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group 2

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alkaline earth metal

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group 18

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noble gases

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group 17

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halogens

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"d" (block elements)

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transition metals

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groups 1,2,13-17 s + p block

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representative elemetns

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"f" block

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inner transition metals

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group/families

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vertical

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periods

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horizontal

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atomic radius

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up and down it increases and left to right decreases

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reason why atomic atomic radius increases going up and down

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reason why atomic radius decreases going left to right

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period trend

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a pattern that changes across a period, yet repeats itself in the next period

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ions

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at atom or a grou of atoms with a charge

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cation

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looses electrons and has a positive charge

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anions

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gains electrons and is a neggative charge

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are metals usually cations or anions?

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cations

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are nonmetals usually cations or anions?

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anions

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which is smaller? (atomic radius) Na +1 or Na

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Na +1

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which is smaller (atomic radius) Cl -1 or Cl

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Cl

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group 1 (charge of ion)

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+ 1

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group 2 (charge of ion)

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+ 2

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group 13

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+ 3

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group 18

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do not form ions

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group 17 (charge of an ion)

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- 1

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group 16 (charge of an ion

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- 2

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group of 15 (charge of an ion)

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- 3

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group 14 (charge of an ion)

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no trend, has metals, nonmetals, and nonmetals

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Ionization Energy

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amount of energy required to remove one electron from an atom in the gaseous state. Increases going left to right and decreases going up to down.

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reaons why the ionization energy decreases going up to down

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reaons why the ionization energy increases going left to right

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first ionization energy

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taking away the last, loose, electron

Front 108

it is harder to take an electron away from Li than K because Li has a higher first ionization energy (closer to than nucleus)

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true

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Units for ionization energy

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K J/ mole

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Octet rule

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atoms will gain, loose, or share electrons to attain an octet--> a full sublevel

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MIDTERM

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MIDTERM