Module 2 - Foundations in Chemistry

mass compared with 1/12th mass of carbon-12

what is the definition of relative isotopic mass?

weighted mean mass compared with 1/12th mass of carbon-12

what is the definition of relative atomic mass?

NO3^-

Nitrate ion formula

CO3^2-

Carbonate ion formula

SO4^2-

Sulfate ion formula

OH^-

Hydroxide ion formula

NH4^+

Ammonium ion formula

Zn^2+

Zinc ion formula

Ag^+

Silver ion formula

PO4^3-

Phosphate ion formula

HCO3^-

Hydrogencarbonate ion formula

H^-

Hydride ion formula

H3PO4

Phosphoric acid formula

HNO3

Nitric acid formula

H2SO4

Sulfuric acid formula

NH4^+

Ammonium ion formula

S8

Sulfur simple molecular formula

P4

Phosphorus simple molecular formula

10^6

How many cm³ in a m³?

10^-6

How many MPa in a Pa?

metal hydroxide + hydrogen

what do a metal + water produce?

salt + hydrogen

what do a metal + acid produce?

salt + water

what do an oxide + acid produce?

salt + water

what do a hydroxide + acid produce?

salt + water + carbon dioxide

what do a metal carbonate + acid produce?

salt + water + carbon dioxide

what do a metal hydrogencarbonate + acid produce?

ammonium salt

what do ammonia + acid produce?

metal oxide + carbon dioxide

what does a metal carbonate produce upon heating?

metal hydrides

When does hydrogen have an oxidation state of -1?

peroxide / -1

what is an example of a situation where oxygen doesn’t have an oxidation state of -2? what is its oxidation state here?

number of electrons needed to be gained or lost to make a neutral atom

what is the definition of oxidation state?

electrons, bonding & structure

2.2 - E__________, B___________ & S___________

sphere

What is the shape of an s orbital?

dumbell

What is the shape of a p orbital?

strong electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms

What is the definition for a covalent bond?

both electrons come from one element

What is dative covalent bonding?

electrostatic attraction between two oppositely charged ions

What is the definition of ionic bonding?

soluble / polar / charged / dissolve

Ionic substances are __________ in water due to the attraction of the _________ water molecule to the __________ ions which pulls them away and they ___________.

dative covalent

Which type of bonding is where there is an arrow signifying electrons come from one element?

linear

What is the shape of this molecule?

trigonal planar

What is the shape of this molecule?

tetrahedral

What is the shape of this molecule?

trigonal bipyramidal

What is the shape of this molecule?

Octohedral

What is the shape of this molecule?

decrease by 2.5

What is the effect of lone pairs on molecule shape?

Pauling scale

What is electronegativity measured with?

an atom’s ability to attract the electron pair in a covalent bond

What is the definition of electronegativity?

increases / decreases

Electronegativity….

• ______________ across periods

• ______________ across groups

covalent / polar covalent / ionic

Place the bond type in order of increasing electronegativity difference (polar covalent, ionic, covalent)

• 0 - _________

• 0 to 1.8 - ________

• >1.8 - _________

difference in charge between two atoms caused by a shift in electron density of the bond

What is the definition of a dipole?

atoms of single element

Which are the only type of molecules that can be purely covalently bonded?

oxygen / fluorine / nitrogen

Which are the elements where hydrogen bonding can occur?

when half or completely full

When is the 3d subshell most stable?

1s^2 / 2s^2 / 2p^6 / 3s^2 / 3p^6 / 4s^2 / 3d^10 / 4p^6 / 4d^10 / 4f^14

What is the order of energy of subshells if they were all full (up to 4f)?

2 / 1s^2

How many electrons fit in shell 1? What is the electron configuration of these subshells?

8 / 2s^2 / 2p^6

How many electrons fit in shell 2? What is the electron configuration of these subshells?

18 / 3s^2 / 3p^6 / 3d^10

How many electrons fit in shell 3? What is the electron configuration of these subshells?

32 / 4s^2 / 4p^6 / 4d^10 / 4f^14

How many electrons fit in shell 4? What is the electron configuration of these subshells?