RULES FOR NAMING ACIDS - CHEMISTRY · Web viewHe found that all matter contained _____ particles...

Name ______________________________________________________ Period_____

Atomic StructureSubatomic particles; development of the atomic theories; atoms, ions and isotopes; average atomic mass;

electromagnetic radiation, EMR calculations

Objective In Class Homework

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Be sure to check the website when you’re absent!

hollickchemistry.weebly.com

Find Someone Who Knows……Question Answer Name (print)

1) What matter is made of

2) The charge of a proton

3) The charge of an electron

4) The charge of a neutron

5) Subatomic particle(s) found in the nucleus

6) Subatomic particle(s) found outside the nucleus

7) Smallest subatomic particle

8) What the atomic number stands for

9) The definition of an isotope

10) The definition of an ion

Parts of an Atom The subatomic particles and their propertiesDraw an atom here name abbreviation

(symbol) location relative mass (in amu) charge

Which subatomic particle:

Determines an element’s identity?

Varies in isotopes?

Varies in ions?

Determines an element’s reactivity?

Has no mass?

Elements are_______________________________________________________________________________

17 atomic number is

Cl a chemical symbol is

35.453 atomic mass is

Atomic Theory History2

Mass number Atomic number

In 1808, _______________________ proposed the 5 Postulates of his Atomic Theory:1. Every element is made of _________________________________________

_____________________________________________________________

2. Atoms of the same element _______________________________________

3. Atoms cannot be _______________________________________________

4. Atoms can combine in ___________________________ to form molecules.

5. Chemical reactions are atoms being ________________________________

____________________________________

In 1890, _______________________ used cathode ray tube experiments to learn more about the atom.

He found that all matter contained _____________________ particles that were

smaller than _____________________ atoms, which were the smallest particles

known to exist. Which of Dalton’s postulates did this disprove? __________

In 1911, he developed a model of the atom that contained these _____________

embedded in a base of ___________________ charge to account for the fact that

matter is usually ________________(not charged). He called this the

______________________________________________.

In 1911, __________________ conducted the ________________________ Experiment that revolutionized the

model of the atom. He fired a beam of __________________________ at a thin sheet of __________________.

A fluorescent screen that detects _______________________ was placed around

the apparatus. By studying where the alpha particles hit the fluorescent screen, he:

Determined that the atom is mostly __________________________________

Established that the nucleus is a ____________________________________

_________________________ region.

In later experiments, he determined that the nucleus contains ________________.

_______________ _______________

In 1913, ______________ was working for Rutherford studying the placement of

____________________ in hydrogen atoms. He discovered that electrons exist in

__________________________________ at varying distances from the atom’s

_______________. He created an ____________________ model of the atom

that we call a Bohr Model.

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Drawing of this model of an atom:




IonsIons are atoms that have gained or lost electrons. #p+ ≠ #e-

Ions are indicated by writing the element’s symbol and the + or – value written as superscript. Ex.___________A cation _________ electrons and has a ____ charge. #p+ #e Examples:_______________________

An anion _________ electrons and has a ____ charge. #p+ #e-

Examples:________________________

HOW TO NAME CATIONS: name(charge) HOW TO NAME ANIONS: name with –ide suffix

Pb2+ = _______________________________ Example: S2- = sulfide Cu+ = ________________________________ Find charge based on periodic table column Cu2+ = _______________________________

Cl = __________________________________Exceptions No roman numerals needed for Group IA, IIA, and CdZnAgAl O = __________________________________

Cd___ Zn___ Ag___ Al ___ N = __________________________________

Na+ = ________________________________ Br = __________________________________

Cd2+ = _______________________________ Naming Practice:

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Partner A: fill in the blanks for an atom of M n+22556

e-______

In hyphenated isotope notation:

Partner B: fill in the blanks for an atom of B r−13581

e-______


p+___n0___

p+___n0___This is a(n)

_______ionThis is a(n) _______ion

Isotopes-Definition: Hyphen Notation

Isotope Notation

Sage and Scribe: You and your shoulder partner must complete at least 8 Petri Dish Atom Models. One partner is sage (tells other what to write); other is scribe (write only in your packet). Switch roles after each dish.

Dish #

# p+

(red)# e-

(black)# n0

(white)Is it an anion,

cation, or neutral?Net

chargeMass

NumberHyphenated Isotope

Notation(name-mass #)

Nuclear Isotope Notation

atomic ¿mass ¿ ¿ Symbol¿

Practice- Isotopes and IonsElement Symbol Atomic

NumberMass

Number# of

Protons# of

Neutrons# of

ElectronsCharge

Oxygen-16 16 0

Ru- 58 +2

26 56 23

35 17 -1

34 18 -2

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Partner A: fill in the blanks for an atom of M n+22556

e-______


Partner B: fill in the blanks for an atom of B r−13581

e-______


Nitrogen-15 8 10

Li- 4 +1

6 12 6

108 47 0

Lead-207 125 78

Atomic Mass (Weighted Average)Atomic Mass = (mass of isotope × decimal of percent) + (mass of isotope × decimal of percent) +…

Or Atomic Mass = (%A x mass #A) + (%B x mass # B) + …..100

Example: There are three isotopes of neon found on the earth: 90.92% is Neon-20; 0.2571% is Neon-21; and 8.822% is Neon-22. What is the average atomic mass of Neon?

Atomic mass = (20 × 0.9092) + (21 × 0.002571) + (22 × 0.08822) = 18.1840 + 0.053991 + 1.94084 = 20.1788 (rounded to the least number of sigfigs based on %)

Practice Atomic Mass1. Magnesium has three isotopes. Magnesium-24 has a 78.70% abundance; magnesium-25 has a 10.13% abundance; and magnesium-26 has a 11.17% abundance. Calculate the atomic mass. Show your work!

2. Mystery element X has two isotopes: 10X (20%) and 11X(80%). What is element X?

3. Please use the following table to calculate the average atomic mass of chlorine.

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Isotope % Abundance Mass(amu)35Cl 75.78% 34.96937Cl 24.22% 36.966

4. Raiderium (Rr) has three naturally occurring isotopes. Raiderium is 74.655% 44Rr, which has an atomic mass of 43.064 amu, 24.958% 46Rr, which has a mass of 46.125 amu, and 0.387% 48Rr, which has an atomic mass of 47.982 amu. Calculate the average atomic mass of Raiderium.

What he did: Experiment using ___________________ in Cathode Ray Tubes.

He studied the spectrum of ____________ emitted when _______________ are excited. He found distinct

emission lines which meant that the electrons exist in ____________________________ rather than

randomly in the electron cloud.

His Contribution: He created a __________________________________ model of the atom that we call a _________________ Model.

Energy Level:

Photon:

Absorption

Emission:

Quantum:

The Bohr Model of Electron Configuration: Draw the electrons on the correct ground state energy levels.

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The Bohr Model of the Atom

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Element: Helium atom Element: Lithium atom Element: Neon atom Element: Phosphorous atomSymbol: _____ Symbol: _____ Symbol: _____ Symbol: _____ Atomic Number: ____ Atomic Number: ____ Atomic Number: ____ Atomic Number: ____# of electrons: ____ # of electrons: ____ # of electrons: ____ # of electrons: ____

The Spectrum of Electromagnetic Radiation (EMR)

All EMR travels at the speed of light, which is __________________.The EMR with the shortest wavelength is ______________ and the longest wavelength is ________________The spectrum of visible light is between ______________ and ____________ on the EMR spectrum.

When ʎ is short (small number),

When the ʎ is long (big number),

Converting nm to meters:1x109 nm = 1 m

The visible light spectrum is given in _______________________While the EMR spectrum is given in ________________________

**Always convert to METERS first**Conversion PracticeA1. Use the fractions above to convert 670 nm to m.

A2. Determine what type of radiation this is_____________ Does this have high/low energy? _____________

B1. Covert 748 nm to meters.

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(Expanded from above)

redorangeyellowgreenblueviolet

B2. Determine what type of radiation this is_____________ Does this have high/low energy? _____________

EMR Equations- equations calculating properties of photons

c= λυ describes the wavelength and speed of a photon with regards to speed of light

c-

λ-

ν -E=hυ describes the energy of a photon with regards to its frequency

E-

h-

ν-

6. What is the frequency of electromagnetic radiation having a wavelength of 212.6 m? (1.41 x 106 )

7. Suppose your favorite AM radio station broadcasts at a frequency of 1.15 x 106 Hz. What is the wavelength, in meters, of the radiation from the station?

8. What is the frequency of blue light that has the wavelength of 4.52 x 10-7 m? (6.64 x 1014)

9. In the flame test, the CuCl2 released green-blue light with the energy of 4.1436 x 10-19 Joules. What was the frequency of this light? (6.25 x 1014)

10. What is the energy of a gamma ray that has the frequency of 5.26 x 1020 s-1? (3.49 x 10-13)

11. What is the frequency of a gamma ray? Gamma rays have a wavelength of 1.001 x 10-14 m.

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The Bohr Model meets the Quantum Mechanical Model

Erwin Schrödinger created the Quantum Mechanical Model described in Schrödinger’s equation a differential equation used to describe how wave functions evolve over time. It uses probability to determine where in 3D space the electron is occupying. It identifies _______________________ on each energy level. Sublevels are composed of ___________________,

which can hold ____ electrons.https://www.angelo.edu/faculty/kboudrea/general/quantum_numbers/Quantum_Numbers.pdf

Quantum Numbers: Principle Quantum Number:

Angular Momentum:

Magnetic:

Spin:

Electron configuration: Rules governing ground state locations of electrons:

Pauli Exclusion Principle Hund’s Rule Aufbau Principle

Example. Atomic Number: __11__ Element: ___Sodium______________ Symbol: ___Na_____

Shorthand Notation: 1s22s22p63s1 Orbital Notation:

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↑↓ ↑↓ ↑↓

↑↓ ↑↓ ↑

1s 2s 2p 3s

https://www.angelo.edu/faculty/kboudrea/general/quantum_numbers/Quantum_Numbers.pdf

Noble Gas Notation: [Ne] 3s1

Whole Class Practice. Atomic Number: __28__ Element: _____________________ Symbol: ________

Shorthand Notation: Orbital Notation:

Noble Gas Notation:

12. A) Atomic Number: ____ Element: _______________________ Symbol: _________

Electron ConfigurationsB) Shorthand Notation: C) Orbital Notation:

D) Noble Gas Notation:




14. A) Atomic Number : ____ Element: _______________________ Symbol: _________Electron ConfigurationsB) Shorthand Notation: C) Orbital Notation:


Valence Electrons- Electrons in the highest energy level and reside on the outer part of the atom. VE are the sum of all the electrons on the _____________ energy level. For representative elements, you can determined it by _________ number.

Shade the representative elements on the PT and label each group with the correct # of VE.

Practice: Write out the shorthand notation for the following elements. Circle their valence electrons.Carbon:

Titanium:

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1s 2s 2p

c

Lewis Dot StructureAlso called Dot Diagrams, these show the element symbol surrounded by the valence electrons. Much like Hund’s rule, when you are placing the electron “dots” around the symbol, you put 1 on each side of the element before putting 2 on any side. For example, the fictional element, Elementium (El) has 3 valence electrons.

Wrong way Right way!

Create a Lewis dot structure for that element in its space on the periodic table below.1 18

1 H 2 13 14 15 16 17 He

2 Li Be B C N O F Ne

3 Na Mg Al Si P S Cl Ar

4 K CaTransitionElements

Ge Ga As Se Br Kr

5 Rb Sr In Sn Sb Te I Xe

6 Cs Ba Tl Pb Bi Po At Rn

7 Fr Ra

Forming Ions Elements are chemically stable with full s and p sublevels in their valence energy level. How many electrons is this?____

Octet Rule: _________________________________________________________________________

Write out the Orbital Diagram for each of the following neutral atoms:Neon Magnesium Fluorine

Which has full valence s and p sublevels?_______________________

Which would be full if it gained one electron?________________________

Which would be full if it could lose its valence electrons and use the s and p underneath? __________________


Electron Configurations

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●●

El ●

●

El ● ●

B) Shorthand Notation: C) Orbital Notation:








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Frequently Used Roman Numerals1 2 3 4 5 6

Iron Symbol_______ Atomic number__________ Starting from this Noble gas, write ORBITAL notation for electrons 19-26

[Ar]Iron (II), Fe__+ forms when it loses the 2 electrons in ______.

Iron (III), Fe__+ forms when it loses _____________________________.

Titanium Symbol_______ Atomic number__________ Starting from this Noble gas, write ORBITAL notation for electrons 19-22

[Ar]Titanium (II), Ti__+ forms when it loses the 2 electrons in ______.

Titanium (IV), Ti__+ forms when it loses _____________________________.

Zinc Symbol_______ Atomic number__________ Starting from this Noble gas, write ORBITAL notation for electrons 19-30

[Ar]Zn__+ forms when it loses its ______ electrons. It has no other stable options, so it does not get a Roman numeral.

Cadmium does the same thing with its 5s electrons, so it is always Cd__+.

Copper Symbol_______ Atomic number__________ Starting from this Noble gas, write ORBITAL notation for electrons 19-29

[Ar]Copper (II), Cu__+ forms when it loses the 2 electrons in ______.

Copper (I), Cu__+ forms when it moves an s electron to the d sublevel and loses the remaining s.

Silver Symbol_______ Atomic number__________ Starting from this Noble gas, write ORBITAL notation for electrons 37-47

[Kr]Ag__+ forms when it moves one of its 5s electrons to 4d, then loses remaining electron in 5s.

It has no other stable options, so it does not require a Roman numeral.

The s block metals and the CdZnAgAl 4 are the only ones that do not get Roman numerals in their names. Aluminum has no d electrons, so its only oxidation state is Al3+.Practice: Write the symbol and charge OR the name with Roman numeral (if required).Cadmium Gold (I) Ni+2 Hg1+

Lead (II) Tungsten (VI) Al+3 Mn4+

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Transition metals: juggling electrons in the d blockTransition metals have electrons in d sublevels that do not count as valence electrons, but can affect how the metal forms cations. Transition metals can lose all, some, or none of their d electrons depending on the reaction environment. Additionally, they can move s electrons into a d orbital if it makes them more stable. The actual number of electrons they lose is called their oxidation state. Because each metal has multiple oxidation states, they are named with their oxidation state as a Roman numeral in parentheses immediately after their name.

Bismuth (V) Platinum (II) Cr+6 W+5

Tin (II) Tin (IV) Cr+3 Pt+4

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Element or Ion Orbital Diagram Electron Configuration

# of Valence Electrons

1 Sn

2 Ni

3 Kr

4 Ra

5 Te

6 S-2

7 Zr+4

8 As-3

9 Ga+3

10 K+

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Element or Ion Orbital Diagram Electron Configuration

# of Valence Electrons

11 Co+2

12 Sn+4

13 Sc+2

14 V+5

15 Mn+2

16 O-2

17 Cu+

18 Cd+2

19 Si4-

20 Co3+

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