Презентация Periodic Table and Trends онлайн
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- Всего слайдов:20 слайдов
- Для класса:1,2,3,4,5,6,7,8,9,10,11
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Слайды и текст к этой презентации:
№1 слайд
Содержание слайда: Periodic Table & Trends
№2 слайд
Содержание слайда: History of the Periodic Table
1871 – Mendeleev arranged the elements according to: 1. Increasing atomic mass 2. Elements w/ similar properties were put in the same row
1913 – Moseley arranged the elements according to: 1. Increasing atomic number 2. Elements w/ similar properties were put in the same column
№3 слайд
Содержание слайда: Group Names
№4 слайд
Содержание слайда: S & P block – Representative Elements
S & P block – Representative Elements
Metalloids (Semimetals, Semiconductors) – B,Si, Ge, As, Sb, Te (properties of both metals & nonmetals)
Columns – groups or families Rows - periods
№5 слайд
Содержание слайда: Periodic Groups
Elements in the same column have similar chemical and physical properties
These similarities are observed because elements in a column have similar e- configurations (same amount of electrons in outermost shell)
№6 слайд
Содержание слайда: Periodic Trends
Periodic Trends – patterns (don’t always hold true) can be seen with our current arrangement of the elements (Moseley)
Trends we’ll be looking at:
Atomic Radius
Ionization Energy
3. Electronegativity
№7 слайд
Содержание слайда: Atomic Radius
Atomic Radius – size of an atom
(distance from nucleus to outermost e-)
№8 слайд
Содержание слайда: Atomic Radius Trend
Group Trend – As you go down a column, atomic radius increases
As you go down, e- are filled into orbitals that are farther away from the nucleus (attraction not as strong)
Periodic Trend – As you go across a period (L to R), atomic radius decreases
As you go L to R, e- are put into the same orbital, but more p+ and e- total (more attraction = smaller size)
№9 слайд
Содержание слайда: Ionic Radius
Ionic Radius –
size of an atom when it is an ion
№10 слайд
Содержание слайда: Ionic Radius Trend
Metals – lose e-, which means more p+ than e- (more attraction) SO…
Cation Radius < Neutral Atomic Radius
Nonmetals – gain e-, which means more e- than p+ (not as much attraction) SO…
Anion Radius > Neutral Atomic Radius
№11 слайд
Содержание слайда: Ionic Radius Trend
Group Trend – As you go down a column, ionic radius increases
Periodic Trend – As you go across a period (L to R), cation radius decreases,
anion radius decreases, too.
As you go L to R, cations have more attraction (smaller size because more p+ than e-). The anions have a larger size than the cations, but also decrease L to R because of less attraction (more e- than p+)
№12 слайд
Содержание слайда: Ionic Radius
№13 слайд
Содержание слайда: Ionic Radius
How do I remember this?????
The more electrons that are lost, the greater the reduction in size.
Li+1 Be+2
protons 3 protons 4
electrons 2 electrons 2
Which ion is smaller?
№14 слайд
Содержание слайда: Ionic Radius
How do I remember this???
The more electrons that are gained, the greater the increase in size.
P-3 S-2
protons 15 protons 16
electrons 18 electrons 18
Which ion is smaller?
№15 слайд
Содержание слайда: Ionization Energy
Ionization Energy – energy needed to remove outermost e-
№16 слайд
Содержание слайда: Ionization Energy
Group Trend – As you go down a column, ionization energy decreases
As you go down, atomic size is increasing (less attraction), so easier to remove an e-
Periodic Trend – As you go across a period (L to R), ionization energy increases
As you go L to R, atomic size is decreasing (more attraction), so more difficult to remove an e-
(also, metals want to lose e-, but nonmetals do not)
№17 слайд
Содержание слайда: Electronegativity
Electronegativity- tendency of an atom to attract e-
№18 слайд
Содержание слайда: Electronegativity Trend
Group Trend – As you go down a column, electronegativity decreases
As you go down, atomic size is increasing, so less attraction to its own e- and other atom’s e-
Periodic Trend – As you go across a period (L to R), electronegativity increases
As you go L to R, atomic size is decreasing, so there is more attraction to its own e- and other atom’s e-
№19 слайд
Содержание слайда: Reactivity
Reactivity – tendency of an atom to react
Metals – lose e- when they react, so metals’ reactivity is based on lowest Ionization Energy (bottom/left corner) Low I.E = High Reactivity
Nonmetals – gain e- when they react, so nonmetals’ reactivity is based on high electronegativity (upper/right corner)
High electronegativity = High reactivity
№20 слайд
Содержание слайда: Metallic Character
Properties of a Metal – 1. Easy to shape
Conduct electricity 3. Shiny
Group Trend – As you go down a column, metallic character increases
Periodic Trend – As you go across a period (L to R), metallic character decreases (L to R, you are going from metals to non-metals
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