Periodic Table

Give an example of a transition metal and describe one of its uses and properties.

Describe one real world application of the reactivity series (e.g, in metal extraction or corrosion prevention.)

If you add a piece of zinc to a solution of copper sulphate, the zinc will replace the copper in the compound because zinc is more reactive than copper

Give an example of metal displacement reaction, and explain what happens

Magnesium displaces copper from a solution of copper sulfate

Why are all alkaline earth metals less reactive than alkali metals?

It takes more energy to remove two valence electrons from alkaline earth metals than one valence electron from alkali metals.

How does the melting point trend differ between metals and non-metals in the periodic table?

In general, metals have higher melting points than non-metals.

What happens during a metal displacement reaction between iron chloride and calcium.

calcium, being more reactive, will displace iron from its compound

Draw the electron dot diagram for a single atom of oxygen (0)

Draw the electron dot diagram for chlorine (CI) molecule showing covalent bonding.

What type of bonding occurs in H20, and how is it shown in an electron dot diagram.

polar covalent bonds

Explain how covalent bonds are formed between two non-metal atoms using HCI as an example

a hydrogen atom and a chlorine atom each contribute one electron to a shared pair, forming a single covalent bond.

List two properties each of substances with ionic and covalent bonds.

ionic= High melting and boiling points, conduct electricity when dissolved or melted. covalent=Low melting and boiling points, Poor conductors of electricity.

Why do ionic compounds typically have high melting points compared to covalent compounds

they are held together by strong electrostatic forces between ions

Why do ionic compounds typically have high melting points compared to covalent compounds

they are held together by strong electrostatic forces between ions

Describe how atomic radius changes across a period and down a group in the periodic table.

decreases across a period (left to right) and increases down a group (top to bottom)

What is metallic character, and how does it vary across the periodic table.

a measure of an element's ability to lose electrons and form positive ions,

Use the periodic table to compare the reactivity of potassium (K), magnesium (Mg), and zinc (Zn).

Potassium is the most reactive, followed by magnesium, and then zinc.

Name one alkali metal and describe a key property and use of it.

sodium (Na).

What is a metalloid? Give one example and a common use

An element that is not a metal but that has some properties of metals.

explain why noble gases are chemically

•Elements in the same group all have-

the same number of valence (outer shell) electrons. 

Group 1=

the alkali metals 

Group 2-

the alkaline earth metals

Group 16=

the chalcogens / the oxygen family

Group 17 = the halogens

the halogens

•Group 18 =

the Noble gases

Periods are the

horizontal rows

Groups, or families, are the

vertical arrangements of elements (1-18)

atomic number 

is the number of protons in an atom.

Where are the mass number and atomic number on an element

Mass number on top, Atomic number on bottom.

The mass number

is the total number of protons and neutrons in the nucleus (nucleons).

Number of neutrons =

Mass number – Atomic Number

Number of electrons =

Atomic number

• isotopes=

Atoms of the same element with different numbers of neutrons.

 transition metal block.

The block of elements in the middle of the table.

All metals are:

•Shiny when polished  : e.g., silver jewelries, gold trophies

•Good conductors of heat, electricity, sound

•e.g., copper wires for electricity

•Ductile meaning, they can be made into wires

•Malleable meaning, they can be bent or shaped into sheets.

Transition metal examples-

•Some common transition metals are:

•Iron (Fe)

•Copper (Cu)

•Zinc (Zn)

Titanium (Ti)

Lanthanides and Actinides

Bottom of the periodic table.

Alkali elements all have how many valence electrons

1 valence electron.

Alkali metals become more or less reactive as you go down the group-

Alkali metals become more reactive as you go down the group.

Reactivity for non-metals goes

less reactive

Reactivity for metals

becomes more reactive

Metallic character

Pattern down a group increases, and pattern across a period decreases.

Valence electrons

Electrons in the outmost shell

Electrons all have _____ charge

negative

The inner shell can hold ___ electrons

2

The 2nd shell can hold _____ electrons

8

The 3rd shell can hold______ electrons

18

The 4th shell can hold ______ electrons

32

•When an atom loses or gains 1 (or more) e’s, it forms

an ion (a charged atom).

The total charge =

the number of protons (in the nucleus) – the number of electrons (in the shells)