QUESTION IMAGE
Question
6 remplis le tableau.
| ia (alcalins) exemple | ii a (alcalino-terreux) | iii a | iv a | va | via | vii a (halogènes) | viii a (gaz inertes) | |
|---|---|---|---|---|---|---|---|---|
| b) tendance à perdre ou à gagner des électrons? | perdre 1e⁻ | perdre 2e⁻ | perdre 3e⁻ | perdre ou gagner 4e⁻ | gagner 3e⁻ | gagner 2e⁻ | gagner 1e⁻ | aucun |
| c) ions formés par les éléments de la 3ᵉ période du tableau périodique. | na⁺ |
7 donne la formule chimique la plus probable des ions formés par les éléments suivants.
To fill in the table for part (c) (ions formed by elements of the 3rd period of the periodic table) based on the groups (IA to VIII A):
For Group II A (alkaline - earth metals, valence electrons = 2, tendency to lose 2e⁻):
The element in the 3rd period of Group II A is Magnesium (Mg). When it loses 2 electrons, it forms $\boldsymbol{Mg^{2+}}$.
For Group III A (valence electrons = 3, tendency to lose 3e⁻):
The element in the 3rd period of Group III A is Aluminum (Al). When it loses 3 electrons, it forms $\boldsymbol{Al^{3+}}$.
For Group IV A (valence electrons = 4, tendency to lose or gain 4e⁻; in the 3rd period, Silicon (Si) can form ions, but more commonly, for simple ion formation, we consider the trend. However, in the context of this table (following the pattern of losing/gaining to achieve noble gas configuration), Silicon can form $\boldsymbol{Si^{4+}}$ (losing 4e⁻) or $\boldsymbol{Si^{4 - }}$ (gaining 4e⁻), but since the previous groups (IA, IIA, IIIA) are losing electrons, we can put $\boldsymbol{Si^{4+}}$ (or note that Si can also form covalent bonds, but for the ion - formation pattern here, this follows the losing trend).
For Group V A (valence electrons = 5, tendency to gain 3e⁻):
The element in the 3rd period of Group V A is Phosphorus (P). When it gains 3 electrons, it forms $\boldsymbol{P^{3 - }}$.
For Group VI A (valence electrons = 6, tendency to gain 2e⁻):
The element in the 3rd period of Group VI A is Sulfur (S). When it gains 2 electrons, it forms $\boldsymbol{S^{2 - }}$.
For Group VII A (halogens, valence electrons = 7, tendency to gain 1e⁻):
The element in the 3rd period of Group VII A is Chlorine (Cl). When it gains 1 electron, it forms $\boldsymbol{Cl^{-}}$.
For Group VIII A (noble gases, valence electrons = 8, no tendency to gain/lose electrons):
The element in the 3rd period of Group VIII A is Argon (Ar). It is a noble gas, so it does not form ions (or we can write $\boldsymbol{Ar}$ as it exists as neutral atoms).
So the filled - in table for part (c) (ions formed by 3rd - period elements) would be:
| Group | IA (alcalins) | II A (alcalino - terreux) | III A | IV A | VA | VIA | VII A (halogènes) | VIII A (gaz inertes) |
|---|
(Note: For Group IV A, the ion formation can be a bit more complex as Silicon often forms covalent compounds, but the above follows the pattern of electron gain/loss based on valence electrons for the purpose of this table.)
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To fill in the table for part (c) (ions formed by elements of the 3rd period of the periodic table) based on the groups (IA to VIII A):
For Group II A (alkaline - earth metals, valence electrons = 2, tendency to lose 2e⁻):
The element in the 3rd period of Group II A is Magnesium (Mg). When it loses 2 electrons, it forms $\boldsymbol{Mg^{2+}}$.
For Group III A (valence electrons = 3, tendency to lose 3e⁻):
The element in the 3rd period of Group III A is Aluminum (Al). When it loses 3 electrons, it forms $\boldsymbol{Al^{3+}}$.
For Group IV A (valence electrons = 4, tendency to lose or gain 4e⁻; in the 3rd period, Silicon (Si) can form ions, but more commonly, for simple ion formation, we consider the trend. However, in the context of this table (following the pattern of losing/gaining to achieve noble gas configuration), Silicon can form $\boldsymbol{Si^{4+}}$ (losing 4e⁻) or $\boldsymbol{Si^{4 - }}$ (gaining 4e⁻), but since the previous groups (IA, IIA, IIIA) are losing electrons, we can put $\boldsymbol{Si^{4+}}$ (or note that Si can also form covalent bonds, but for the ion - formation pattern here, this follows the losing trend).
For Group V A (valence electrons = 5, tendency to gain 3e⁻):
The element in the 3rd period of Group V A is Phosphorus (P). When it gains 3 electrons, it forms $\boldsymbol{P^{3 - }}$.
For Group VI A (valence electrons = 6, tendency to gain 2e⁻):
The element in the 3rd period of Group VI A is Sulfur (S). When it gains 2 electrons, it forms $\boldsymbol{S^{2 - }}$.
For Group VII A (halogens, valence electrons = 7, tendency to gain 1e⁻):
The element in the 3rd period of Group VII A is Chlorine (Cl). When it gains 1 electron, it forms $\boldsymbol{Cl^{-}}$.
For Group VIII A (noble gases, valence electrons = 8, no tendency to gain/lose electrons):
The element in the 3rd period of Group VIII A is Argon (Ar). It is a noble gas, so it does not form ions (or we can write $\boldsymbol{Ar}$ as it exists as neutral atoms).
So the filled - in table for part (c) (ions formed by 3rd - period elements) would be:
| Group | IA (alcalins) | II A (alcalino - terreux) | III A | IV A | VA | VIA | VII A (halogènes) | VIII A (gaz inertes) |
|---|
(Note: For Group IV A, the ion formation can be a bit more complex as Silicon often forms covalent compounds, but the above follows the pattern of electron gain/loss based on valence electrons for the purpose of this table.)