Untitled Quiz

Study Notes

MgCl2 is Magnesium Chloride; it is ionic with an electronegativity difference of 1.8.
Fe2O3 is Iron (III) Oxide; identified as ionic with an electronegativity difference of 1.7 and involves a transition metal.
Ti2O is Titanium (I) Oxide; considered ionic because of its electronegativity difference of 2.0.
Ammonium Phosphate has the formula (NH4)3PO4; it is ionic due to the presence of polyatomic ions.
Rubidium Iodide is identified as ionic due to the absence of prefixes in its name.
KMnO4 contains both ionic and covalent bonds; the ionic bond exists between potassium and the permanganate ion, while the bond between manganese and oxygen is covalent.

NO2 is Nitrogen Dioxide; it is covalent with an electronegativity difference of 0.5, indicating polar characteristics.
Ge3P4 is Trigermanium Tetraphosphide; it is covalent with a non-polar electronegativity difference of 0.3.
Sb2Te5 is Diantimony Pentatelluride; a covalent compound marked by an electronegativity difference of 0.3.
CCl4 is Carbon Tetrachloride, also covalent with an electronegativity difference of 0.5.
Disilicon Hexafluoride with the formula Si2F6 is identified as covalent due to its use of prefixes.

Ionic compounds generally dissolve in water and dissociate into ions; they conduct electricity when dissolved.
Some covalent compounds may dissolve in water, but they do not dissociate into ions and typically do not conduct electricity.
Covalent substances can melt at lower temperatures compared to ionic compounds, which require high temperatures to melt.
Ionic compounds are solid at room temperature, whereas covalent compounds can exist as gases or liquids.
In solid form, ionic compounds are brittle; covalent compounds can be malleable.

The term "polar" in covalent bonds denotes a situation where there is a slight charge difference, whereas "non-polar" indicates even sharing of electrons.
The suffix "ate" in names indicates the presence of a polyatomic ion, impacting naming conventions for ionic compounds.