mrs. valentine's math and science · web view2.1 atomic structure and models objective: i will...

Unit 2 – Atomic Structure Name: ____________________________

2.1 Atomic Structure and Models

Objective: I will be able to label/draw an atom. I will understand the progression of the atomic models. I will be able to identify differences in isotopes of the same element.

Vocabulary:

Electron Proton Neutron Nucleus Electron CloudDalton Model Thomson Model Rutherford Model Bohr Model Cloud ModelOrbit Orbital Isotopes Nuclides Mass NumberAtomic Number

Notes:

Atomic models o __________ Model (1803) – hard ________ different for each

substanceo Thomson’s Model (a.k.a. ________ ________Model) – negative

particles called _______________ surrounded by positive matter o _________________ Model (1911) – Central positive

______________ surrounded by electrons moving randomlyo ___________ Model (1931) – Arranged the electrons in circular

_________ with ___________ ____________ around the nucleuso __________________ Model (1926) – Electrons occupy orbitals

(areas of _____ probability of finding electrons) around nucleus Anatomy of an Atom

o Nucleus _____________

_____________ charged subatomic particles __________ _______________ – # protons; determines element

_____________ – neutral subatomic particles These two particles are approximately the same ___________ and ___________

o Electron Cloud ___________ – _______________ charged subatomic particles (very small;

_____________ the mass of a proton) Moving at very __________ ______________ Electrons exist in ______________ according to current model

________________o Atoms of the ___________ ____________ with __________________ ____________o ______________ – an isotope of an elemento _______________ numbers of __________________; all same properties except ______o __________ _______________ is number of ____________ and __________ combinedo Symbols:

C612

o Some isotopes are ____________________ (too much ___________ in nucleus)


2.2 Bohr Models & Dot Diagrams

Objective: I will be able to draw and read Bohr models and dot diagrams of the atoms and ions of the first eighteen elements.

Vocabulary:

Valence Electrons Dot Diagrams Ion Valence Electrons

Notes:

Bohr Modelso Inaccurate model for all but ________________ in terms of how the atoms

____________, but Bohr models provide an easy ___________ of what’s going on with the _________________.

o On the _________-_________ ring, you can only put ______ electronso On the __________ _____ rings, you can put up to ______________ each. o Always fill the diagrams _____________ from the ________________o The electrons on the outer-most occupied ring are called ____________ ____________

A ______________ atom can have between ___ and ___ valence electrons _____________, ________, or _____________ in order to form compounds.

Valence electrons _____, ________ outer electrons Valence electrons _______, ________ outer electrons

An ______ is an atom that has __________ or _______ __________ __________ If charge is _____________, ________ that number of valence electrons If charge is _____________, ________ that number of valence electrons

Dot Diagramso Uses the ____________ of the element in the __________, surrounded by ________

representing _______________ _____________o There are _______ sides of the symbol: ____, _________, _________, _______. o Pick a side to start on and put ______ electron on each side ___________ ___________

up (obviously ____________ when you have ___________ _____ the valence electrons). o Examples

Aluminum: Oxygen: Bromium: Hydrogen:


2.3 Periodic Trends

Objective: I will be able to identify the groups of the periodic table. I will understand the trends of valence electrons, oxidation numbers, and reactivity on the periodic table.

Vocabulary:

Reactivity Periodic Table Group Period HalogensTransition Metals Actinides Alkali metals Alkaline Earth

MetalsOxidation Numbers

Noble Gases Lanthanides Rare Earth Metals

Notes:

Periodic Tableo A chart used to organize the ______ known ______________o __________________

Created the ____________ periodic table by organizing the elements by their ____________________

Accurate enough to correctly ________________ the existence of __________ _________________ elements and their properties

o Reading the blocks of the periodic table Each square has

Element _____________ Element __________ ____________ ____________ Average atomic __________

Each ______ is in numerical order of _____________ __________ _____________________ of the Periodic Table

o Groups ____________ of the periodic table Numbered _________, or ____ thru _______ for the __________ columns and

_________ for the _____________ columns Elements are _________________ together by having similar properties Specific Groups

_____________ Metalso Group ___; ____ valence electrono _____________ reactive metals (_________ reactive)o __________, __________o Do not exist as elements in nature (only as part of compounds)

_____________ __________ Metalso Group ___; ____ valence electronso ______________ most reactive metals o Soft, gray (slightly _____________ than group ____ metals)o Do not exist as elements in nature (only as part of compounds)


__________________ Metalso Groups _______o ________ are _____________, some are ______o ____________ ___________ for some (such as gold and copper)o Most ______________ thought of metals are transition metals

__________ ___________ Metalso Not part of a ___________ (____ rows ________ periodic table)o ____________________

_______ of bottom two rows Soft, malleable, shiny, conductive, ______________ to

separateo ____________________

______________ of bottom two rows Only _____ are ____________ (thorium and uranium);

all others are ________________ Some only last ______________ of a _____________

before they ___________ down _____________ Groups

o Groups _______ are considered mixed groups because they have __________, ____________, and ____________ in them.

o The ______________ for these groups will _____ be as _____________ as other groups are.

o Named after the _______ ____________ in each group.o The Groups:

___________ Group – Group ___; ___ valence electrons ___________ Group – Group ___; ___ valence electrons ___________ Group – Group ___; ___ valence electrons ___________ Group – Group ___; ___ valence electrons

_____________o Group ____; ___ valence electronso ________ ______________ nonmetals (mostly)o Pure halogens are _________________ to humans

___________ ____________o Group ____; ___ valence electronso ________________o _____________ at room temperature

o ____________ _______ of the periodic table There are _____________ from top to bottom Elements in a period have _________ properties from others in the same period

____________ Electronso The number of valence electrons an element has is related to its group number (for

groups _______, ___________)


o Number of valence electrons equals the _________-place of the __________ number _______________ Numbers

o Oxidation number is the number of __________________ that an atom __________ or __________ when it becomes an ______.

o __________ to the ion’s ___________o For __________, the number of __________ ______________ ___________ the

_______________ number, because metals _________ their electrons when they form ________ (_______________ a ______________ leaves a _______________ charge)

o For ______________, the oxidation number equals the ____________ of _____________ the nonmetal will ___________ when they form ________.

To find this value, __________ ________ from the number of valence electrons. This will be a ____________ number because nonmetals gain negative electrons

Shade and label the periodic table. Include a legend at the bottom.


2.4 Ionic Compounds

Objective: I will be able to identify ionic compounds based upon their composition. I will understand the general properties of ionic compounds.

Vocabulary:

Ionic Compound Ionic Bond Anion Cation Polyatomic IonsCrystal

Notes:

________________o ______ bonds form when ions of _________________ charges attract each other.

__________ are ions with a _____________ charge _________ are ions with a _____________ charge

o Electrons are _________________o Occur between a ______________ and a __________o __________ compounds are always ___________, meaning that the ________

__________ charge is ________ to the _______ ___________ chargeo ______________ _______

Made of _____ or _______ atoms _________ together Work as a ____________ ________ Behave in the same way that ______________ ions do

Propertieso __________ Shape

Ions are packed together in an ________________ ___________ Crystal

an orderly, ________-______________ arrangement of atoms or ions in a __________

tend to have __________ ________ for a single compound different ___________ for different ______________

Break into ______-_________ when struck by a hammer due to alternating ionso High _____________ _____________

__________ must be _____________ to ________ an ionic solid Ex: NaCl – _________

o ________________ ___________________ Ions have electric charge, but as a __________, they ___________ conduct

_________________ Bound _____ _________ together When ____________ in water, they ___________ _____________ and separate,

allowing _____________ to _______ through The __________ ____________ applies to _________ ionic substances


2.5 Ionic Nomenclature

Objective: I will be able to name ionic compounds from their formulas and write the formulas of ionic compounds from their names.

Vocabulary:

Nomenclature

Notes:

________________ is a ______________ _____________. Formula to Name

o Reading Formulas The ____________ of any compound ________ the ____________ that are

bonded by their ___________. For ________ compounds, the _________ is listed ________ followed by the

___________. ________________ after each symbol indicate _______ __________ of the ions

are present in the _____________ _________-______________ ________.

o Naming Formulas Name the ______________ ________ without changing its name. The

___________ is _____ part of the name. If the cation is a ______________ metal or has __________ _____ _____

oxidation number, ___________ the __________ number as ____________ ________ in _________________ after the name.

Name the _________ by _____________ the __________ to ______. Exception: if the anion is a _____________ _____, keep the name as is.

Example: FeBr3 is ___________________ K2S is _______________________ LiNO3 is ____________________

Name to Formulao From each part of the name, write the ____________ for the corresponding ion. o If one of the ions is __________, put its symbol in __________________ before you

continue.o To ensure that the formula is _____________, take the __________ of the __________

and make it the _____________ of the _______. Take the _____________ ________ of the _____________ of the _________ and make it the ____________ of the ___________.


o ____________ the _____ ____________, as ionic formulas are in the simplest whole-number ratio.

o Examples: Calcium fluoride

Iron(III) carbonate

Strontium Oxide


2.6 Molecular Compounds

Objective: I will be able to identify molecular compounds based upon their composition. I will understand the general properties of molecular compounds.

Vocabulary:

Covalent Bond Polar Nonpolar Double Bond Triple BondMolecular Compound

Notes:

Compositiono A ___________ bond is a bond formed when two atoms _________ electronso Made of _______ or more ______________o ___________ Bonds

________ bonds – _____ pairs of shared electrons _______ bonds – ________ pairs of shared electrons

o _______________ compounds have ________________ bonded atoms Exist as ______________ ______________ ______________ between molecules are ___________ than ionic bonds _____________ molecules share electrons ____________ ________ molecules have an _________ share of electrons (a ___________

__________ and a ____________ ____________ end)

__________ works using polarity:

Propertieso Molecules can be small (______ _________ – ex: CO) to huge (____________ of atoms –

ex: DNA)o Have ______ ___________ points and __________ pointso ________ conductors of ______________o When molecular compounds _____________, molecules

______________ from one another, but remain _____________ unitso Polar substance _______________ in polar solvents while nonpolar

substance dissolve in nonpolar solvents. (like dissolves like)


2.7 Molecular Nomenclature

Objective: I will be able to name molecular compounds from their formulas and write the formulas of molecular compounds from their names.

Notes:

Formula to Nameo Reading Formulas

For molecular compounds, the ________________ after each symbol indicate ______ ________ __________ of that element are in _______ ______________.

Subscripts are ______ ______________ to their simplest whole-number

o Naming Formulas For molecular compounds, the ______________ are _________ of the

____________ as a ____________ before each element’s name. Prefixes

Number Prefix Number Prefix1 62 73 84 95 10

If the element’s name begins with an “___” or an “___”, then the prefix __________ the “___” or “___” from the _______

The _________ element Uses the appropriate numerical prefix from above (except “________”). Keeps its _______ __________

The second element listed still uses the prefix, but changes its suffix to “______” Examples:

C3H8 N2O5 CBr4

Name to Formulao Pick out the ______________ in the ________________, and use the _____________ to

determine ______ _________ atoms of each _____________ there are. o List them in the __________ _______________ as the name.o Examples:

Tetranitrogen monoxide Diboron hexahydride Iodine heptafluoride


2.8 Metallic Bonds

Objective: I will understand the properties of metallic bonds.

Vocabulary:

Metallic Bond Sea of Electrons

Notes:

The __________ that holds _________ _____________ in a _______________ substance Atoms are _____________ ___________

_______________ energy ___________ ______________ between atoms Valence electrons are _________________, moving ___________ throughout the space

_________________ ______________ ________ _____ ________________ – the body of ________________ ______________ that

surround ______________ metal ions in _________________ _________o Allows atoms to __________ __________ each other ____________ without breaking

bonds (explains _________________ and __________________)o Allows _______________ through the ____________ easily (good _______________ of

_______________)o Light __________ ________________ the metal ______________ (___________)


2.9 Mixed Nomenclature

Objective: I will be able to identify if a substance is ionic, molecular, or metallic, and then I will be able to name it or write its formula accordingly.

Notes:

Always determine the _________ _____ ________________ __________! Then use the _________________ ________________ system Practice

Ionic/Covalent? Name Formula

Tin(II) Nitrate

Strontium Fluoride

Gold (II) Oxide

Sulfur Dichloride

Silver Oxide

Calcium Phosphate

Mercury (II) Bromide

Phosphorus Trifluoride

Ammonium Sulfate

SiCl4

N2O

BaSO4

Na3PO4

ZnO

Mg(OH)2

P4O10

LiC2H3O2

(NH4)2Se

mrs. valentine's math and science · web view2.1 atomic structure and models objective: i will...

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