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Welcome to SNC2D!. Review Game. Chemistry Review Game. Early Model of The Periodic Table. SNC2D Review: The Periodic Table. Mendeleev's Arrangement of the elements:. 1860s Dimitri Mendeleev organized the elements looking for patterns

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review game
Review Game
  • Chemistry Review Game
slide4

SNC2D Review: The Periodic Table

Mendeleev's Arrangement of the elements:

  • 1860s Dimitri Mendeleev organized the elements looking for patterns
  • He organized elements (50 known at that time) according to atomic mass into the "periodic table" since he noticed patterns periodically
  • When organized this way, he could predict properties of the known elements - he left "gaps" in the table where he felt elements were missing
slide5

The modern Periodic table:

  • Today's periodic table is based on increasing atomic number (# of protons)
  • Each elements has a symbol, name, atomic number, atomic mass and possible ion charges
  • Elements 1 - 93: naturally occur. The remaining elements are synthetic (and often not stable)
slide6

Periods and Groups

  • Period: A horizontal row on the periodic table (1-7)
  • Group: A vertical column on the periodic table (1-18)
  • A group is also called a family since elements in groups have similar chemical and physical properties
  • Well known groups: alkali metals, alkaline-earth metals, halogens and noble gases
periodic table

18

17

Period

Group

1

2

1. Alkali Metals

2. Alkaline Earth Metals

17. Halogens

18. Noble Gases

Periodic Table
slide8

Classes of Elements in the Periodic Table:

  • Metals: Elements on the left side of the periodic table (except H)
  • Metals: Solid (except Hg), Shiny, conduct heat and electricity, malleable and ductile
  • Non-Metals: Elements on the right side of the periodic table
  • Non-Metals: gases & solids, not shiny, poor conductors of heat and electricity, brittle and not ductile
  • Metalloids: on diagonal line between metals and non-metals
  • Metalloids: Share properties with metals and non-metals
slide9

SNC2D Review: Standard Atomic Notation

  • Standard atomic notation: mass number is always on top of the atomic number

Calculating the number of subatomic particles:

  • Atomic number = # protons
  • Mass number = # protons + # neutrons (round!)
  • # neutrons = mass number - atomic number
  • # protons = # electrons
slide11

SNC2D Review: Bohr-Rutherford Diagrams

  • According to the Bohr-Rutherford model of the atom, electrons occupy energy levels or "shells"
slide12

SNC2D Review: Bohr-Rutherford Diagrams

  • Electrons in farther from the nucleus have more energy compared to those closer to the nucleus
  • Each shell can hold a different amount of electrons (2, 8, 8, 2) for the first 20 elements
  • We represent elements using Bohr-Rutherford diagrams
slide13

Drawing Bohr-Rutherford diagrams:

  • Draw a circle for the nucleus, indicate the number of protons and neutrons in the circle

2) Determine the # of electrons for that atom - draw bigger circles around the nucleus to represent shells

3) Starting with the shell closest to the nucleus, place small circles to represent electrons on the energy shells (2, 8, 8, 2)

4) Write the name of the element under the diagram

bohr rutherford diagram
Bohr-Rutherford Diagram

73Li

3p+

4no

lithium

bohr rutherford diagram1
Bohr-Rutherford Diagram

199F

9p+

10no

fluorine

slide16

Drawing Bohr-Rutherford diagrams:

  • Draw a circle for the nucleus, indicate the number of protons and neutrons in the circle

2) Determine the # of electrons for that atom - draw bigger circles around the nucleus to represent shells

3) Starting with the shell closest to the nucleus, place small circles to represent electrons on the energy shells (2, 8, 8, 2)

4) Write the name of the element under the diagram

slide20

6P6N

Examples of Bohr-Rutherford Diagrams

Carbon