Chemistry Flashcards
What is a cation?
An ion with a positive charge
(tip: think of cats -> positive!)
What is an anion?
An ion with a negative charge
How to name binary acids?
Hydro________ic acid
How to name ternary oxacids ending in -ate?
-ate ->_______-ic acid
(tip: I ATE an ICky bug)
How to name ternary oxacids ending in -ite?
-ite -> ______-ous acid
(tip: SprITE is deliciOUS)
What is the formula for density?
Density = mass(g) /volume(mL)
What is the unit for density?
g/mL
What is the unit for volume?
mL
What is the unit for mass?
g
Define the octet rule
Atoms are the most stable with 8 valence electrons
Name the types of intramolecular forces
Ionic bonds and covalent bonds
Name the types of intermolecular forces (IMFs) in order of strongest to weakest
Ion-dipole forces
Hydrogen bonding
Dipole-Dipole
London Dispersion Forces (LDFs)
What element(s) must be bonded to hydrogen to create a hydrogen bond?
Fluorine
Oxygen
Nitrogen
(tip: think of the acronym FON)
What is different about the elements that create ionic bonds and covalent bonds?
Ionic bonds are created with non-metals and metals
Covalent bonds are formed with ONLY non-metals
What are the two criteria for a molecule to become polar?
Must have at least one polar bond
Must be asymmetrical
(tip: asymmetry appears when the central atom has one or more lone pairs or if there are different elements surrounding the central atom)
Which is stronger: single bonds or triple bonds?
Triple bonds!
Which is longer: single bonds or triple bonds?
Single bonds!
What happens to electrons during ionic bonding (where do they go)?
Electrons are transferred between the elements to create negatively or positively charged ions
What happens to electrons during covalent bonding (where do they go)?
Electrons are shared between elements until all elements satisfy the octet rule
What are the steps in creating a Lewis Structure?
1) determine the type and number of electrons
2) add up the total number of valence electrons
3) arrange the atoms as symmetrically as possible
4) place the valance electrons around the atoms to reach a filled octet
Define the Valence Shell Electron Pair Repulsion Theory (VESPR)
Because electrons are negative, they will repel each other
-> this helps predict the molecular shape and electron pair geometry
What is the difference between electron-pair geometry and molecular shape?
Electron-pair geometry looks at all places with electron-pair domains, so, both lone pairs and bonds
Molecular shape only looks at the atoms surrounding the central atom
In a molecule with two atoms around the central atom and NO LONE PAIRS, what is its molecular shape and bond angle?
Linear and 180
In a molecule with one atom around the central atom and NO LONE PAIRS, what is its molecular shape and bond angle?
Linear and there is no bond angle
(because there is no second atom to create an angle)
In a molecule with two atoms around the central atom and ONE LONE PAIR, what is its molecular shape and bond angle?
Bent and >120
(because the electron-pair geometry is trigonal planar and the VESPR theory means that the two bonded atoms will move away from the lone pair)
In a molecule with two atoms around the central atom and TWO LONE PAIRS, what is its molecular shape and bond angle?
Bent and >109.5
(because the electron-pair geometry is tetrahedral and the VESPR theory means that the two bonded atoms will move away from the lone pair)
In a molecule with three atoms around the central atom and NO LONE PAIRS, what is its molecular shape and bond angle?
Trigonal planar and 120
In a molecule with three atoms around the central atom and ONE LONE PAIR, what is its molecular shape and bond angle?
Trigonal pyramidal and >109.5
(because the electron-pair geometry is tetrahedral and the VESPR theory means that the two bonded atoms will move away from the lone pair)
In a molecule with four atoms around the central atom and NO LONE PAIRS, what is its molecular shape and bond angle?
Tetrahedral and 109.5
