PV=nRT⇒P=(nRV)T⇒P=kT  where,k=(nRV)  or  T=k′P  where,k=1k′

The geometric structure and the physical and chemical properties of atoms, ions, and molecules usually do not depend on their physical state; the individual water molecules in ice, liquid water, and steam, for example, are all identical. In contrast, the macroscopic properties of a substance depend strongly on its physical state, which is determined by intermolecular forces and conditions such as temperature and pressure.

Electrons in bonding molecular orbitals help stabilize a system of atoms since less energy is associated with bonded atoms as opposed to a system of unbound atoms.  Bonding orbitals are formed by in-phase combinations of atomic orbitals and increase the electron density between the atoms (see figure 2 below)   Electrons in antibonding molecular orbitals cause a system to be destabilized since more energy is associated with bonded atoms than that of a system of unbound atoms. Antibonding orbitals are formed by out-of-phase combinations of atomic orbitals and decrease the electron density between atoms (see figure 2 below). 

fig. 9.2.5: Boron ground state electron configuration on left, and the hybrid orbital configuation on the right that is involved with the three bonds in boron trifluoride. 

fig. 9.2.4:  Beryllium is also sp hybridized in beryllium chloride. What is the orbital of the chlorine in BeCl2? it is a 3p orbital as chlorine has one free-radical orbital in it's valence state, and so there is no need to hybridize it.

A bond in which the electronegativity of B (χB) is greater than the electronegativity of A (χA), for example, is indicated with the partial negative charge on the more electronegative atom: lesselectronegativeAδ+−moreelectronegativeBδ−(8.4.1)(8.4.1)lesselectronegativemoreelectronegativeA−Bδ+δ− \begin{matrix} _{less\; electronegative}&  & _{more\; electronegative}\\   A\; \;  &-& B\; \; \; \; \\  ^{\delta ^{+}} & & ^{\delta ^{-}} \end{matrix} \tag{8.4.1} ​

Oxidation is the loss of electrons Reduction is the gain of electrons

3.5: Acid-Base Reactions

BaCl2 (aq)

Ag2SO4 (aq)

Pb+2(aq)+ 2 NO3-(aq) + 2 Na+(aq)+ SO4-2(aq) 2 NO3-(aq)+ 2Na+(aq)+ PbSO4(s)

6 NH4+(aq)

Ca(OH)2

Na3PO4

Ca(CO3)2

Ag(s)

CaCO3(s) -->   CaCO(s) + CO2(g)  As the name implies, something decomposes into something else.  Here Calcium Carbonate decomposes to calcium oxide and carbon dioxide

(aq) - aqueous

Problems

2.38 kg

Students at UALR need to know the common names for the above metals with variable oxidation state.  

homonuclear diatomic ion

Natural States of Atoms