The Periodic Table

Oxygen

Fluorine

Phosphorus

Neon

Oxygen

Carbon dioxide

Hydrogen

Chlorine

Fluorine

Chlorine

Bromine

Iodine

1

2

3

4

$Na, Si, Cl$

$Cl, Si, Na$

$Li, Na, K$

$S, P, Si$

It becomes more negative (more exothermic) as the attraction for electrons increases.

It becomes less negative (less exothermic) as the atoms get smaller.

It remains constant because the shielding is the same.

It decreases as the nuclear charge increases.

It increases because the number of electrons increases.

It decreases because the effective nuclear charge increases.

It remains constant because all electrons are in the $n=2$ shell.

It increases then decreases as you reach the noble gas.

Element $X$ is $Al$; Element $Y$ is $Mg$; Element $Z$ is $S$

Element $X$ is $Mg$; Element $Y$ is $Na$; Element $Z$ is $P$

Element $X$ is $Si$; Element $Y$ is $Al$; Element $Z$ is $Cl$

Element $X$ is $Al$; Element $Y$ is $Na$; Element $Z$ is $Si$

Increasing nuclear charge

Increasing atomic radius and shielding

Decreasing number of energy levels

Increase in effective nuclear charge

$NaCl$ dissolves to form a solution with pH 7.

$AlCl_3$ reacts to form a solution with pH 12.

$SiCl_4$ does not react with water.

$PCl_5$ reacts to form a solution with pH 7.

$Na + H_{2}O \rightarrow NaOH + H_{2}$

$2Na + 2H_{2}O \rightarrow 2NaOH + H_{2}$

$Na + 2H_{2}O \rightarrow Na(OH)_{2} + H_{2}$

$2Na + H_{2}O \rightarrow Na_{2}O + H_{2}$

Acidic

Alkaline

Neutral

Organic

It increases

It decreases

It stays the same

It fluctuates

It sinks and remains at the bottom

It fizzes steadily and disappears

It burns with a bright green flame

It creates a loud sonic boom immediately

Dull and black

Shiny and silvery

Rough and brown

Blue and translucent

$Li_2CO_3$

$Na_2CO_3$

$K_2CO_3$

$Rb_2CO_3$

Sodium metal

Sodium ions

Hydrogen atoms in water

Hydroxide ions

Stability increases down the group as the $M-H$ bond becomes more ionic

Stability decreases down the group as the $M-H$ bond enthalpy decreases

All hydrides are equally stable

Hydrides cannot be decomposed thermally

$K_2O$ (Oxide)

$K_2O_2$ (Peroxide)

$KO_2$ (Superoxide)

The $O-O$ distance is the same in all

$Li^+$

$Na^+$

$K^+$

$Cs^+$

They become lighter

They become darker

The color disappears

They all turn blue

Gas

Liquid

Solid

Aqueous

$Cl_2 + 2Br^- \rightarrow 2Cl^- + Br_2$

$Br_2 + 2Cl^- \rightarrow 2Br^- + Cl_2$

$Cl + Br \rightarrow ClBr$

$Cl_2 + Br_2 \rightarrow 2ClBr$

The atoms become smaller

The nucleus is further from the incoming electron and more shielded

The boiling point increases

They have more valence electrons

$Br_{2} + 2Cl^{-} \rightarrow 2Br^{-} + Cl_{2}$

$I_{2} + 2Br^{-} \rightarrow 2I^{-} + Br_{2}$

$Cl_{2} + 2F^{-} \rightarrow 2Cl^{-} + F_{2}$

$Cl_{2} + 2Br^{-} \rightarrow 2Cl^{-} + Br_{2}$

It decreases because the atomic volume increases faster than the mass.

It increases because the atomic mass increases more significantly than the atomic volume.

It remains constant because they are in the same group.

It increases because they change from gas to liquid to solid.

Iodine

Bromine

Chlorine

Fluorine

$Cl \cdot$

$CH_{3} \cdot$

$Cl^{+}$

$Cl^{-}$

It is a gas at room temperature.

Its $H-At$ bond is stronger than the $H-I$ bond.

Silver astatide ($AgAt$) is soluble in dilute ammonia.

It is a poorer oxidizing agent than iodine.

$F^{-}$

$Cl^{-}$

$Br^{-}$

$I^{-}$

Titanium

Sodium

Lead

Barium

+1

+2

+3

+4

Iron

Nickel

Platinum

Vanadium

Platinum

Titanium

Calcium

Palladium

Copper

Cobalt

Iron

Chromium

Nickel

Iron

Platinum

Vanadium

Electrons moving between energy levels in the d-subshell

The presence of water molecules acting as ligands

The size of the metal nucleus

The number of neutrons in the isotope

Scandium

Manganese

Zinc

Iron

$Ti^{3+}$

$V^{3+}$

$Zn^{2+}$

$Mn^{2+}$

To reduce the iron ore to iron metal.

To react with acidic impurities like $SiO_2$ to form slag.

To provide the fuel for the high-temperature reactions.

To act as a catalyst for the reduction of carbon dioxide.

Fuel for rockets

Shielding gas for arc welding

Bleaching agent for paper

Catalyst for ammonia production

Helium

Argon

Xenon

Radon

Flammable

Non-flammable

Highly explosive

Only flammable in oxygen

$Ar_2$

$Ar$

$Ar_8$

$Ar_3$

It decreases because the nucleus becomes stronger.

It increases as the number of electrons increases and the electron cloud becomes easier to distort.

It remains zero because the atoms are symmetrical.

It decreases because the atomic radius increases.

Argon

Helium

Radon

Xenon

Xenon has more valence electrons.

Xenon has a lower first ionization energy due to greater shielding and distance from the nucleus.

Xenon is more electronegative than Neon.

Neon's nucleus is larger, making it more stable.

Bond order 1, Paramagnetic

Bond order 0, Diamagnetic

Bond order 0, Paramagnetic

Bond order 1, Diamagnetic

Concentrated $HCl$

Concentrated $H_2SO_4$

Dilute $HNO_3$

Hydrofluoric acid

It has the lowest ionization energy of the noble gases

It emits a characteristic bright orange-red light when an electric discharge passes through it

It is the most abundant noble gas in the atmosphere

It is highly reactive and forms colorful ions easily