Periodic, Atomic size, and Groups trends
Isoelectrons and Shielding
Ionization (IE, Trends, Successive ionization, Ionization and reactivity Trends)
Alkalai Metals, Halogens, Electronegativity
I dont know how to categorize the rest
100

Which 3 factors influence the Atomic size. Explain

Atomic size is influenced by 1. Energy Level The higher energy level is further away the shell is. 2. Charge on nucleus More charge pulls electrons in closer. 3. Shielding effect The first shell weakens the pull to the second shell and so on

100
Define an isoelectronic ion
An iselectronic ion is when two ions have the same electronic structure and same number of valence electrons.
100

describe what happens to ionization energy of atoms as it move down group 1.

As it moves down group 1, IE becomes less

100
Define electronegativity. And state what atom halogen atoms is the bases to compare electronegativity.
A measure of the ability of an atom to attract electrons in a covalent bond F
100

Electronic configuration of Phosphorus?

1s2 2s2 2p6 3s2 3p3

200

What happens to the atoms as we go down the groups. Explain

As we go down a group each atom gains another energy level so the atoms get bigger.

200
What happens to the size of isoelectronic ions which have more protons
Isoelectronic ions that have more protons are smaller.
200

Define First Ionization energy(100) and write the equation for second ionization.(100)

Amount of energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of ions.(100) Na+(g) - Na2+(g) + e- 2nd ionization of sodium Not Na(g) - Na2+(g) + 2e- (100)

200
Define equation of reaction of Alkali metals with water. And State which metal has the most reactivity
2X(s) + 2H2O(l)-->2XOH(aq) + H2(g) Fr
200

Complete this sentence: The oxides become .... ...... as ... go ...... ... ......

The oxides become more acidic as you go across the period.

300
What happens to the ions as you go down the groups. Explain
By going down the group you are adding an energy level as a result the ions get bigger
300
In a valence shell which electron is shielded most the second electron or the first electron. Explain
Both are shielded the same amount as the pull from the nucleus is the same on every electron in one valence shielded or not
300

In the Chemistry class, Jamie is having a experiment to know about Ionization Energy. His metal needed loads of energy to remove 3rd electron. If he used the metal in group 2, Evaluate whether this experiment was successful or not.

Successful. since the electrons of group 3 metals need to jump over the shell, it needs loads of energy.

300
State 3 features of the group of atoms which can be cut my knife.
Most are silvery metals Too reactive to be found as elements in nature Shiny, smooth surfaces when freshly cut
300

Do ionic compounds have high or low melting points. Explain

They have high melting points as the ionic compounds have ionic bonds which require a lot of energy to break

400
What happens to the radius as you go across the period and why
As you go across a period, the radius gets smaller because the nuclear charge increases and as a result all the outermost electrons that are in same energy level get pulled closer to the nucleus
400
Fully and clearly explain the phenomenon know as shielding
When the pull from the nucleus on the electrons of the outer valence shells decreases due to the energy required to hold the electrons in the previous valence shells in place
400

one of the halogen atom has the most reactivity. Define the atom.(100) However, it needs a friend for the christmas. If the most reactivity halogen atom want to be less reactivity with its girlfriend, then what will atom in group 1 be ideal friend for christmas?(100) and justify reason. (200)

F. Li. Since it has the least reactivity, It make a less reactivity by ionization.

400
If the diatomic atom is very reactive and has red brown color, Distinguish its electronegativity with another diatomic atom whose color is green.
Basically, comparison between Br and Cl. Compare to F, Cl has less difference of EN than Br. Thus, Cl has more electronegativity than Br.
400

definition of the term first ionization energy

The energy required to remove one mole of electrons from one mole of gaseous atoms.

500
For the two Statements bellow state which isotope is bigger - Li1+ has 2e and 3p whist Be2+ has 2e and 4p. - N3- has 10e and 7p whilst O2- has 10e and 8p,
Be2+ has a greater nuclear charge than Li1+ and so is smaller. N3- has a greater nuclear charge than so O2- is smaller
500
Are these are Isoelectronic ions. Explain -CO -N2 -NO+
CO, N2 and NO+ are isoelectronic because each has 2 nuclei and 10 valence electrons (4+6, 5+5, and 5+5)
500

Arrange in a order of biggest atom. and Justify your answer. N. S. Na. I. B.

We don't know. Since we don't know exact value of how much electronegativity has been affected to the atoms.

500

Noble Gases do not have electronegtivity except for?

Xenon and Radon

500

Which oxides are acidic?

P4O10 , SO3, ClO2

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