Week Two Flashcards
PV= nRT
P= pressure V= volume N= amount of substance R= gas constant T= temp
Accuracy
How close the value is to the correct value
Precision
How reproducible a particular measurement is when made a number of times
Significant figures
Writing in scientific notation shows how many significant figures are present
Significant figures - key concepts
All nonzero digits are significant
When zero is significant
- between two nonzero digits
- at the end of a number that includes a decimal point
When a zero is not significant
- before the first nonzero digit in a number
- at the end of a number with a decimal point
Chemical formula
Shows the number of each type of atom present in a substance
Molecular formula
Refers to a discrete molecule, describes the types a number of atoms present in a molecule
Binary compounds
Compounds containing only 2 elements
Binary compounds naming rules
- With exception to hydrogen, elements further to the left of the periodic table are first
- If hydrogen is present, it appears last with elements from group 16 and 17
- both elements from same group, lower one goes first
Structural Formula
Shows the ay in which atoms are bonded together to form molecules
Isomers
Molecules that have the same chemical formula but different chemical structures
Condensed structural formula
Arranged in bonded groups but actual bonds aren’t drawn
Cis
Ch3 on same side
Trans
Ch3 on different sides
Naming non metallic binary compounds
Element closest to the left appears first
The second element begins with elemental name but ends with the suffix -ide
Naming oxoanions
Name has the root of central atoms
When the element forms more than one oxoanion then the one with fewer oxygen ends in -ire and the other has -ate
Alcohols
Have -oh (hydroxyl) group attached to a carbon
Naming: -ol
Aldehyde
Have carbonyl (c=o) group
Is always bonded to at least one hydrogen
Must be end of carbon chain
Naming: -anal
Ketones
Always bonded to two other carbon atoms
Never end of chain
Carboxylic acid
Carboxyl group (-cooh) can only bind to one other atom End of chain
Alkanes
Single bond
Saturated
Formula - CnH2n+2
Molecular equation
It shows all reactants and products, with molecular substances written as discrete molecules (i.e.HCl,H2OandCO2) and ionic compounds written in terms of their empirical formulae (i.e.CaCO3andCaCl2)
Empirical Formula
simplest whole-number ratio of atoms within that compound. For example, the empirical formula of butane (chemical formulaC4H10) isC2H5.
