Periodic Table Flashcards
Name the trends across a period from left to right
- Number of protons increases
- Atomic radius decreases
- Metallic properties decreases
Name the trends down a group from top to bottom
- Number of protons increases
- Number of electron shells increases
- Atomic radius increases
- Metallic properties remain constant
Where are transition metals found in the periodic table?
Between Group II and Group III (except zinc)
Name 3 physical properties of transition metals
- high melting and boiling points, and high densities due to strong metallic bonds
- good electrical and thermal conductors
- form coloured compounds
Name 1 important chemical property of transition metals
- Have the ability to exhibit multiple oxidation states, hence transition metals and their compounds are often used as catalysts
Where are alkali metals found in the periodic table? Why are they called alkali metals?
Group I elements. Because they react with water to give alkaline solutions.
Name 3 physical properties of alkali metals
- low melting and boiling points compared to other metals
- low densities compared to other metals and less dense than water
- good conductor of electricity and heat
The atomic radius of alkali metals increase down the group, causing ________ to increase down the group, and ________ to decrease down the group.
Densities; melting points
Why does reactivity of alkali metals increase down the group?
Down the group, electron shells increase and the nucleus is further away, which increases the ease of losing the single valence electron
What are halogens?
Elements in Group VII of the periodic table. They usually exist as diatomic molecules.
Name 4 physical properties of halogens
- low melting and boiling points that increases down the group
- coloured
Why does reactivity of halogens decrease down the group?
As size of atom increases, it becomes more difficult for the nucleus to draw an additional electron into its valence shell
Name the 3 physical properties of noble gases
- colourless and odourless
- very low melting and boiling points but increase going down the group
- insoluble in water
Why are noble gases unreactive and inert?
They have complete electronic structures/ fully filled valence shell. They are unreactive and inert since they have a stable electronic configuration.
