Unit 1: Periodic Table Flashcards
Atomic Number
No. of protons
Relative Atomic Mass
Protons + Neutrons mass/Nucleolus mass
Isotopes
Same element with different Mass no/R. atomic mass (or changes in no of neutrons)
Excited Electrons
When electrons gain enough energy to jump shells
What happens with an Electron returns to its shell after jumping shells?
It produces an Electromagnetic wave that leads to Electromagnetic Radiation.
It can be heat, light, ultraviolet waves, etc.
Ionisation
The act of an electron gaining enough energy to move out of the atom
Ionizing Radiation
An energy that ionizes an atom or removes an electron
Give an example of Ionizing Radiation
X-rays
They penetrate our bodies by removing electrons from the area they pass
Also present in soil, water and vegetation
Why do groups have similar properties?
They have the same no. of electrons
Physical Properties of Metals
Good conductors
High melting and boiling points
Metallic Luster (shiny)
Malleable and Ductile (can turn into wires) - because of crystalline atomic structure
Sonorous
Durable (varies)
Best and Worst Metal Conductors
Best - Silver (Ag) and Copper (Cu)
Worst - Lead (Pb) and Mercury (Hg)
Chemical Properties of Metals
High Density
Reacts with Oxygen (some burn and some oxidize)
Form positive ion (because they’re more likely to donate electrons given their low valency)
Comment on the Lattice of a Metal
Solid metals are a lattice of positively charged nuclei in a ‘sea’ of mobile electrons or delocalised electrons.
This is what makes metals so conductive, because the delocalised electrons move freely and carry electricity.
What state are Metals found in?
Solid (- Mercury in Liquid)
What state are Non-Metals found in?
All (maybe more gases)
Main Properties of Non-Metals
Opposite of Metals
Good Insulators
Name all the Metals in the Periodic Table
Metals, Transition Metals, Non-metals, Metalloids
Main Characteristic of Transition Metals
Very good catalysts (better at donating and accepting electrons because of their partially filled d-orbit)
Eg. Platinum, Nickel, etc.
Main Characteristics of Metalloids
Semi Conductive
Luster
(not Malleable, Ductile or Durable)
Explain the Application of each of these metals in a Phone
Metals - cover (for Luster/shine and Durability/protection) and wires (Cu)
Metalloids - processor (because the Semi-Conductivity allows electricity to pass in a controlled manner. A metal would allow too much electricity to flow making it short-circuit.)
Non-Metals - battery (non-metals like Li are present in the positive and negative electrodes of a battery. When it chargers, they move to the negative electrode and vice versa. This produces the energy needed.)
Basic Properties of Nobel Gases (Group 8)
Stable/inert - full valence shell
Colorless
Trends in Nobel Gases (Group 8)
Top-to-bottom
(Due to Atomic Radius Increasing) Density increases top-to-bottom - Think concentration
- Melting/boiling Points
Uses of Nobel Gases (Group 8)
Airships (Helium)
Car head light, anesthesia, satellite steering (Xenon)
Lightbulbs (Argon)
Radioactive cancer therapy (Radon)
Glass insulation (Krypton)
Basic Properties Alkaline Metals (Group 1)
Metallic character (Metal properties)
Theyre called Alkaline because when heated with water they produce an Alkaline solution
Reactive, soft, low melting/boiling point, low density
Almost always form an ionic compound
Metal + Water = Compound = Hydrogen gas
How are Alkaline Metals (Group 1) stored?
In oil or under an inert gas like Argon (Noble gas)
Trends in Alkaline Metals (Group 1)
Top-to-bottom
Softer
More reactive
+ Melting/boiling points
(+ density)
Basic Properties Alkaline Earth Metals (Group 2)
Same properties as Group 1
+ Ductile and Malleable
How are Group 1, Group 2 and Group 7 Metals found in nature?
Theyre found in compounds
Where are Alkaline Earth Metals (Group 2) used?
Fireworks, present in our teeth (calcium)
Basic Properties of Halogens (Group 7)
Toxic
They exist as Diatomic Molecules (covalent bonds)
Trends in Halogens (Group 7)
Top-to-bottom
+ Melting/boiling point
+ Density
Uses of Halogens (Group 7)
F - strongest known substance to accept electrons. Used to etch glass, prevent tooth decay, make apatite.
Cl - disinfectants, bleaching agents, paper/wood pulp, salt (for our body).
I - cloud seeing to initiate rain using silver iodide, important for our metabolic rate
Br - Sedatives, other drugs
What is Cloud Seeing?
A weather modification technique that improves a cloud’s ability to produce rain or snow by introducing tiny ice nuclei into certain types of subfreezing clouds
Most cloud seeding operations, use a compound called silver iodide (AgI) to aid in the formation of ice crystals
aka Iodine from Halogens (Group 9)
Used by United Arab Emirates
Halogens + Metals
Metal Halides (eg. salt)
Reactivity Series
Please send lions, cats, monkeys and cute zebras into hot countries - signed Gordon
Potassium, Sodium, Lithium, calcium, magnesium, carbon, Zinc, Iron, Hydrogen, Copper, Silver, Gold
K, Na, Li, Ca, Mg, C, Zn, Fe, H, Cu, Ag, Ar
Trend: Metallic Character
Top right to Bottom left: Increase - because electronegativity
Trend Electronegativity
Top left to Bottom right: Increase - because metals
Electronegativity
The tendency to accept ions
Anion and Cation
Negatively and Positively charged ion
Electron Affinity
Amount of energy released when an anion is made
Trend: Electron Affinity and Ionization Energy
Left to right: Increase
Bottom to top: Increase
Trend: Atomic Radius
Right to left: Increase
Top to bottom: Increase
Trend: Melting and Boiling Point + Nuclear Force
Right to left: Increase
Top to bottom: Increase
Nuclear Force
Attraction between nucleolus and outermost shell
