Significant Figures
Metrics
SI
Conversions
Density
100
Why do we use significant figures
To factor in the precision of our measurement tools
100
What is one benefit to using the metric system for science?
~Measurement intervals are in powers of ten for easier conversion ~Collaboration- it is widely used in other countries
100
What does SI stand for?
Systeme International or the System of International Units
100
What is a conversion factor?
a equivelency that allows you to mathematically change the unit of a measurement without changing the overall value of your measurement
100
What is the formula for density?
D= m/v
200
What are the rules to using significant figures?
1) ALL non-zero numbers (1,2,3,4,5,6,7,8,9) are ALWAYS significant. 2) ALL zeroes between non-zero numbers are ALWAYS significant. 3) ALL zeroes which are SIMULTANEOUSLY to the right of the decimal point AND at the end of the number are ALWAYS significant. 4) ALL zeroes which are to the left of a written decimal point and are in a number >= 10 are ALWAYS significant
200
what is the base unit of measurement used for mass?
grams
200
What is the SI unit for time?
seconds
200
What are the steps for converting?
1. put the number they give you on the outside 2. make your fraction 3. fill in your units (want/have) 4. put the numbers from the conversion factor in the fraction 5. multiply by the top and divide by the bottom to solve
200
What are the units used for density?
g/mL g/cm3
300
How many significant figues are in this number? 0.0407
3
300
What is the base unit of measurement for volume?
Liters
300
What is the SI unit for weight?
Newtons
300
14mm = _____m
0.014m
300
What is the density of an object with a mass of 2.5 g and a volume of 2.03mL?
1.2 g/mL
400
How many significant figures are in this number? 501.040
5
400
How many mm are in 1 cm?
10 mm
400
What is the SI unit for mass?
Kilogram (kg)
400
34kg = _____g
34,000 g
400
What is the density of an object that has a mass of 149.2g and a volume of 130mL
1.1 g/mL
500
Write the answer to this addition problem in significant figures. 2.005 + 0.0430 + 0.14
2.2
500
How many nanoliters are in 1 L?
1,000,000,000 nL = 1L
500
What is the SI unit for amount of a substance?
mole
500
4.2 moles = ____ atoms
2.5 x 10 24
500
What is the mass of an water that has a denisty of 1.00g/mL and a volume of 300.0mL?
300g
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