Scientific Notation & Units Overview

These flashcards provide a comprehensive review of the key concepts related to scientific notation, significant figures, units of measure, and dimensional analysis, as outlined in the lecture notes.

What is scientific notation?

A value written as a number between 1 and 10 multiplied by 10 raised to a power.

What are the two components of scientific notation?

Coefficient (a number between 1 and 10) and Exponential Term (10 raised to a power).

How do you convert a number greater than 10 into scientific notation?

Move the decimal to the left and make the exponent positive.

How do you convert a number less than 1 into scientific notation?

Move the decimal to the right and make the exponent negative.

What is the rule for addition and subtraction with significant figures?

The result should not have more decimal places than the number with the least decimal places.

What is the rule for multiplication and division with significant figures?

The result should have the same number of significant figures as the factor with the fewest significant figures.

Define significant figures.

The digits that carry meaning contributing to a measurement's precision.

What does a trailing zero after a decimal indicate about significant figures?

It is significant.

What does a leading zero indicate about significant figures?

It is not significant.

What is the process of dimensional analysis?

Identify starting units and final desired units, ensuring consistent units throughout calculations.

What is the SI unit for mass?

Kilogram (kg).

What SI prefix represents one million?

Mega (M).

What is the formula for calculating mass based on moles and molar mass?

Mass (g) = Number of Moles (mol) × Molar Mass (g/mol).

How is molarity defined?

The number of moles of solute per litre of solution.

What is a weight/volume percent solution?

The weight in grams of solute per 100 mL of solution.

When performing unit conversions, what is crucial to check?

Ensure that quantities are in the same units for addition/subtraction, and that units are appropriately handled in multiplication/division.

What does the mole concept relate to in chemistry?

1 mole of a substance equals its molecular mass in grams.

What does specific gravity indicate?

Density relative to water, where the density of water is taken as 1 g/mL.

What is the relationship between moles, molarity, and volume in a solution?

Amount (mol) = Concentration (M) × Volume (L).