2. Periodic Vocabulary Atomic Radius Metal Electronegativity
Metalloid Family Noble Gas Group Nonmetal Ionic Radius Periodic Law
Ionization Energy Period 3. Classifying Elements Dmitri Mendeleev
observed that whenthe elements were arranged in order ofincreasing
atomic mass, similar chemicaland physical properties appeared
atregular or periodic intervals. This was later determined to not
exactlybe the case. Modern Periodic Law The properties ofelements
are periodic functions of their atomicnumbers. If the elements are
arranged increasing atomicnumber (not atomic mass) properties are
repeatedperiodically. For the majority of the table it is also
appears as if it is organized by increasing atomic mass, there are
however some 4. Classifying Elements Dmitri Mendeleev observed that
whenthe elements were arranged in order ofincreasing atomic mass,
similar chemicaland physical properties appeared atregular or
periodic intervals. This was later determined to not exactlybe the
case. Modern Periodic Law The properties ofelements are periodic
functions of their atomicnumbers. If the elements are arranged
increasing atomic number(not atomic mass) properties are repeated
periodically. For the majority of the table it is also appears as
if it is organized by increasing atomic mass, there are however
some exceptions. Can you spot them? Ar and K; Co and Ni; Te and I;
Th and Pa, U and Np; Pu and Am; Lr and Rf; Sg and Bh, Hs and Mi 5.
Basic Periodic Table InfoAtomicMass Common oxidation states (ions)
Chemical Symbol Atomic Number Electron configuration 6. Chemical
Symbols Each symbol has one, two, or three letters. First letter is
always capitalized. Other letters (if present) are lowercase.CAu
Uuu 7. Chemical Symbols Each symbol has one, two, or three letters.
First letter is always capitalized. Other letters (if present) are
lowercase.CAu UuuRg 8. Name the movie 9. Arrangement of the
PeriodicTable 10. Arrangement of the PeriodicTable
Metalloids(semimetals) 11. General Characteristics of Element on
the PeriodicTableA. Metals: (Fr = most metallic element)1. All
(except Hg) are solid at room temperature.2. Have luster. (are
shiny)3. Are Malleable (can be pounded into shape)4. Are ductile
(can be drawn into wires)5. Are excellent conductors of heat and
electricity. Due to mobile electrons.6. Have low ionization energy.
Tend to lose electrons7. Have low electro-negativity.and become
postive (+) ions. 12. General Characteristics of Element on the
PeriodicTableB. Nonmetals: (F = most nonmetallic)1. Can be gases,
liquids, or solids. Most nonmetals are gases or solids (molecular
ornetwork) at room temperature. Bromine is a liquid at room
temperature.2. Lack luster. (are dull)3. Are brittle. (crumble
easily)4. Are poor conductors of heat and electricity.5. Have high
ionization energy. Tend to gain electrons6. Have high
electro-negativity. and become negative (-) ions. 13. General
Characteristics of Element on the PeriodicTableC. Metalloids:
(semi-metals)1. Properties are a combination of metallic and
nonmetallic substances. Located along the staircase B, Si, As, Sb,
Te, Po 14. Elements in Nature Some elements can exist as a single
atom in nature, some cannot Monotomic Elements: Most elements exist
as single atom particles in nature. Na, Si, Te, W Diatomic
Elements: Some elements cannot exist as a single atom, instead they
exist as a two atom particle in nature. HOFBrINCls H2, O2, F2, Br2,
I2, N2, Cl2 15. Elements in Nature Allotropes: Some elements exist
as two or more forms in the same phase. These forms differ in
molecular or crystal structure, and hence in their chemical and
physical properties. Allotropes of Oxygen Oxygen (O2) and Ozone
(O3) 16. Elements in Nature Allotropes of CarbonCoal/Graphite
DiamonBuckminsterfullerend e Allotropes of Oxygen Oxygen (O2) and
Ozone (O3) 17. Groups (Families) Vertical columns of elements. Have
similar characteristics due to havingthe same number of valence
electrons. Example;HLi B FNaGroup 1Al Group 13 ClGroup 17K All have
one Ga All have three Br All have sevenRb valence In
valenceIvalenceCselectron.Ti electrons. Atelectrons.Fr 18. Periods
(rows) Horizontal rows of elements. Elements within a period have
the samenumber of occupied principal energylevels. They differ
however, in their chemical properties.Period 1: H, He use the 1st
Principal Energy or 1sLevel Example;Period 2: Li, Be, B, C, N, O,
F, Ne use the 2nd Principal EnergyLevelor 1s2s2pPeriod 3: Na, Mg,
Al, Si, P, S, Cl, Ar use the 3rd PrincipalEnergy Level or 19.
Trends in Properties Atomic Radius: (Table S) Covalent atomic
radius: the distancebetween the nuclei of two atoms of thesame
element joined in the solid phase bya covalent bond. Within a
period, atomic radius decreases. Within a family (group), atomic
radius increases. 20. Group Group Group Group Group 1 Li2 B 3 C 4 O
5 Ne ePeriod2PeriodMg3PeriodCa4 21. Trends in Properties Ionic
Radius: (No Table/ Estimate using tableS) An atom that has gained
or lost electrons,will change in atomic size. Metals tend to lose
electrons, thus the outer shell is lost/pulled closer and the ionic
radius will be smaller than the covalent radius. Nonmetals tend to
gain electrons, thus the outer shell is stretched larger as the
additional electrons start to repel each other and the ionic radius
will be larger than the covalent atomic radius. 22. Practice
Question Which of the following has the greaterionization energy,
Na or Na+?Explain your answer. 23. Practice Question Which of the
following has the greaterionization energy, Na or Na+?Explain your
answer.Na+ has higher ionization energy as ithas 11 protons holding
10 electronswhile Na has 11 protons holding 11electrons. 24.
Summary Within a Period, as atomic numberincreases.1. Covalent
atomic radius_______________2. Ionization Energy _______________3.
Electronegativity _______________4. Metallic Character
_______________Within a group, as atomic number increases.1.
Covalent atomic radius_______________2. Ionization Energy
_______________3. Electronegativity _______________4. Metallic
Character _______________ 25. Summary Within a Period, as atomic
numberincreases.1. Covalent atomic radius decreases Table S2.
Ionization Energy increases3. Electronegativityincreases Periodic
Table4. Metallic Character decreasesWithin a group, as atomic
number increases.Table S1. Covalent atomic radiusincreases2.
Ionization Energy decreases Periodic Table3. Electronegativity
decreases4. Metallic Character increases 26. Do Now Mendeleev
arranged the periodic table inorders of increasing atomic
masses.Locate iodine and tellurium on the table andnote that they
are not arranged byincreasing atomic mass, and yet Mendeleevplaced
iodine in Group 17 and tellurium inGroup 16. What is the likely
reason that hechose not to arrange these two elements byatomic mass
as he did for the majority of hisoriginal table? 27. Do Now
Mendeleev arranged the periodic table inorders of increasing atomic
masses.Locate iodine and tellurium on the table andnote that they
are not arranged byincreasing atomic mass, and yet Mendeleevplaced
iodine in Group 17 and tellurium inGroup 16. What is the likely
reason that hechose not to arrange these two elements byatomic mass
as he did for the majority of hisoriginal table?He placed the
tellurium and iodine into thecolumns of elements with
similarcharacteristics. 28. Chemistry of GroupsAlkali Metals Alkali
Earth (1) Metals (2) 29. Chemistry of Groups Group 1 Alkali Metals
Have one valence electron. Form +1 ions. (complete octet) Highly
reactive. Reactivity increases as one proceeds from top to bottom
of the table (increasing atomic number). Typically form very stable
compounds. Group 2 Alkali Earth Metals Have two valence electrons.
Form +2 ions.(complete octet) Highly reactive. Reactivity increases
as on proceeds from top tobottom of the table (increasing atomic
number).Group 1 and Group 2 element are generally found as
compounds in Typically only very stable compounds.nature, and
usuallyformseparated into elemental form by a process 30. Chemistry
of Groups * *Staircase* * * * 31. Chemistry of Groups Group
13,14,15,16 Staircase Have 3,4, 5, and 6 valence
electronsrespectively. Group 13 forms +3 ions. (Complete octet)
Groups 14, 15, and 16 tend to gain e- and form -4, -3, and -2 ions
repectively. (Complete octet) Properties change from nonmetals
(C/N) tometalloids (Si/As) to metals (Pb/Bi) withincreasing atomic
number.MetalsMetalloidsNonmetals13 14 15 16 13 14 15 1613 14 15 16
B CN OB CN O B CN OAl Si P S Al Si P SAl Si P SGa Ge As Se Ga Ge As
SeGa Ge As SeIn Sn SbIn Sn Sb In Sn Sb TeTe Te 32. Chemistry of
GroupsThe Halogens 33. Chemistry of Groups Group 17 Halogens Have 7
valence electrons. Form -1 ions. (complete octet) Highly reactive
nonmetals. Reactivity decreases with increasing atomic #. Halogen
States of Matter (Room Temperature) F and Cl = gases Br = liquid I
= solid At = No known stable isotopes. This means that all of
itsisotopes are radioactive. *** All elements with an atomic number
above 83 haveno known stable isotopes.*** 34. Practice Question Why
does chemical reactivity increase fromtop to bottom of Group 1,
while it decreasesfrom top to bottom of Group 17? 35. Practice
Question Why does chemical reactivity increase from topto bottom of
Group 1, while it decreases fromtop to bottom of Group 17?Group 1
contains metal which lose electronsand have large atomic radii in
order to have lowionization energy and low electronegativity.Atomic
radius increases as you move from topto bottom of a group.Group 17
contains nonmetals which gainelectrons so smaller atomic radii is
required forhigh ionization energy and highelectronegativity. 36.
Chemistry of GroupsNoble Gases 37. Chemistry of Groups Group 18
Noble (Inert) Gases Have 8 valence electrons. (Complete Octet)
Generally NOT reactive. *** Under extreme conditions Kr and Xe have
beenmade to react with Flouring and Oxygen. This is whythey have
oxidation numbers other than 0.*** 38. Chemistry of
GroupsTransition Metals d sublevel elementsLanthanide Series
Actinide Series f sublevel elements 39. Chemistry of Groups Groups
3 to 12 Transition Metals Generally exhibit positive oxidation
numbers. All contain electrons that are bounced between two outer
principal energy levels; as a result these elements are usually in
a constant semi- excited state. Solutions of these elements are
usually colorful. 40. Chemistry of a PeriodAs one progresses from
left to right along the periodic table: There is a change from + to
oxidation states. There is a change in characteristics from: Very
Less Less VeryNobleReacti ReactiMetalloiReactive Reactive(Inert)ve
veds (Nonmetals (Nonmetals Gases(Metal (Metal) )s) s) 41. Do Now
Elements with atomic number 112 and 114 havebeen produces and their
IUPAC names arepending approval. However, an element that wouldbe
put between these two elements on the periodictable has not yet
been produced. If produced thiselement will be identified by the
symbol Uut until anIUPAC name is approved. Determine the charge of
the Uut nucleus. Include both thenumerical value and the sign of
the charge. Identify one element that would be chemically related
toUut. 42. Do Now Elements with atomic number 112 and 114 havebeen
produces and their IUPAC names arepending approval. However, an
element that wouldbe put between these two elements on the
periodictable has not yet been produced. If produced thiselement
will be identified by the symbol Uut until anIUPAC name is
approved. Determine the charge of the Uut nucleus. Include both
thenumerical value and the sign of the charge.+113 Identify one
element that would be chemically related toUut.Any element of Group
13; B, Al, Ga, In, Tl 43. Using the Periodic Table topredict
Chemical Formulas Water (H2O) is formed by the sharing ofelectrons
so that each atom can try toemulate the outer shell
electronconfiguration of a noble gas (completeoctet) Hydrogen (H)
tries to be like Helium (He) Oxygen (O) tries to be like Neon
(Ne)CovalentBond We will explore this further when we start to
learn about 44. Using the Periodic Table topredict Chemical
Formulas Hydrogen belongs to Group 1 which form+1 ions. Oxygen
belongs to Group 16 which form -2ions. Nonmetal 45. Using the
Periodic Table topredict Chemical Formulas Ice melt (CaCl2) is
formed by the electromagneticattraction between positive ions forms
by a metaland the negative ions formed by a nonmetal. Calcium (Ca)
loses its 2 electrons to become theCa+2 ion in order to be like the
Noble gas Argon(Ar) 2-8-8-22-8-8 2-8-8 Chlorine (Cl) gains an
electron to becom the Cl-1ion in order to be like Argon (Ar) as
well.2-8-8 2-8-72-8-8 46. Using the Periodic Table topredict
Chemical FormulasMetal Nonmetal Ionic Bond 47. Using the Periodic
Table topredict Chemical Formulas Predict the chemical formulas for
the following K+1 P-3 Beryllium and Carbon Mg+2 Cl-1 Cesium and
Fluorine Ca+2 S-2 Group 13 (X) andGroup 16 (M) B+3 O-2 48. Using
the Periodic Table topredict Chemical Formulas What would be the
general formula of aGroup 2 element (represented by M)combined with
chlorine of Group 17? What would be the general formula of agroup
16 element (represented by X)combined with sodium of group 1? 49.
Using the Periodic Table topredict Chemical Formulas In the 19th
century, Dmitri Mendeleevpredicted the existence of a then
unknownelement X with a mass of 68. He alsopredicted thant an oxide
of X would havethe formula X2O3 . On the modern periodictable, what
is the group number and periodnumber of element X. 50. Using the
Periodic Table topredict Chemical Formulas What groups do the
elements of the folwingcompound belong to? Mg3P2 AlBr3 GaN CH4 51.
Isoelectricity Ions and atoms (noble gases) thatcontain the same
number of electrons. Example; K+1, S-2, and Ar are isoelectronic
because they each contain 18 electrons. Ge-4, Br-1, Rb+1, Sr+2, and
Kr are isonelectronic because they contain 36 electrons. 52.
Practice question Ions are isoelectronic when they contain the
samenumber of electrons. Which of the following ionsare
isoelectronic? Mg+2, Cl-1, Al+3, K+, S-2, Ba+2 For each of the
preceding ions name the noblesgas with which they are isoelectronic
with. 53. Metals and Conductivity. In terms of electrons, why are
metalsgood conductors of electricity? The valence electrons of
metals aremobile and form an electron cloudaround the metallic
bonds of a givenmetal element. This cloud of mobile electrons also
serves in the thermal conductivity of metals. 54. To get these
slides go tohttp://mrmartinschemistryblog.blogspot.com
