Chapter 1 Flashcards
Naming covalent vs ionic compounds
Covalent:
use prefixes
end second element in -ide
Ionic:
use roman numerals in ()
end second element in -ide
determining homogeneous vs heterogeneous mixtures from compound
aqueous compounds are ALWAYS homogeneous mixtures
sand (s) and water (aq) for example is ALWAYS heterogeneous
determining physical vs chemical change
Creating something new/changing chemical composition (like burning): chemical change
Visibly see a change/can go back to previous form (like freezing): physical
is… a physical or chemical property?
odor
toxicity
flammability
density
malleability
boiling point
odor: P
toxicity: C
flammability: C
density: P
malleability: P
boiling point: P
which has more PE (stored nrg): solid or gas?
solids have more stored energy/ PE
where does heat transfer
heat always moves from where it’s hot to where it’s not.
if two objects are next to each other and one is cold one is hot then heat will move from hotter to colder object until they have the same temp.
how do you calculate the total NRG of an object?
Total NRG= Kinetic NRG + Potential NRG
energy is never lost just converted from KE –> PE or PE –> KE
Energy vs work
energy: the capacity to do work
work: action of a force through a distance
what does the weight of an object measure? what does mass measure?
mass: measures the quantity OF matter within it
weight: the gravitational pull ON its matter
sig figs when adding/subtracting vs multiplying/dividing
add/sub: least number of dec. places
mult/div: least number of sig figs
ROUND AT THE VERY END!!
scientific law vs theory
law: states how it behaves (summarizes past observations and predicts future ones)
theory: states why it’s happening not merely how it behaves
pure substances vs mixtures
PS: ELEMENT (cannot be broken down into simpler substances includes diatomic**) or COMPOUND (fixed proportion of DIFF elements)
Mixture: Homo (same composition throughout) and hetero (composition varies)
BP and FP of water in C and K
what’s absolute zero?
BP: 100 C and 373 K
FP: 0 C and 273 K
absolute zero: -273 C and 0 K
extensive property
property that depends on the amount of the substance
ex: volume and mass
derived unit
combination of other units
ex: volume, density, speed
what is uncertainty and how do you calculate the uncertainty of a measuring instrument?
uncertainty is how much a measurement varies around an already-measured value
how to calculate: plus or minus (±) half the smallest scale division
ex: for a thermometer with a mark at every 1.0°C, the uncertainty is ± 0.5°C
estimated digit
if marker on a measuring instrument goes by 0.1, 0.2, etc. then the estimated digit would be the number in 0.01, 0.02, etc.
exact numbers
have no uncertainty
random vs systematic error
random: unpredictable, usually human errors–equal probability of being too high or too low
systematic: problem in measurement system–tends toward being EITHER too high or too low
precision vs accuracy
precision: how close a series of measurements are to ONE ANOTHER
accuracy: how close the measured values are to the actual value
converting units raised to a power
raise both the number AND the unit to the power
ex:
2in –> ((2)^2)in^2 –> 4in^2
prefixes 1-10
mono
di
tri
tetra
penta
hexa
hepta
octo
nona
deca
space filling models
represent electron clouds
metals that form cations with different charges
CCC L TMI
Copper (l)
Copper (ll)
Cobalt (ll)
Cobalt (lll)
Chronium (ll)
Chronium (lll)
Led (ll)
Led (lV)
Tin (ll)
Tin (lV)
Mercury (l)
Mercury (ll)
Iron (ll)
Iron (lll)
