Density and the Periodic Table

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Questions and Answers

In an experiment studying plant growth, a scientist varies the amount of fertilizer given to different plants. Which variable is the independent variable?

  • The height of the plants after a month.
  • The amount of fertilizer given to the plants. (correct)
  • The type of plant used in the experiment.
  • The amount of sunlight each plant receives.

A student measures the mass of a rock to be 150 grams and its volume to be 50 cm³. What is the density of the rock?

  • 7500 g/cm³
  • 3.0 g/cm³ (correct)
  • 0.33 g/cm³
  • 100 g/cm³

Which of the following is an example of a chemical change?

  • Boiling water.
  • Burning wood. (correct)
  • Melting ice.
  • Dissolving sugar in water.

If an atom has 11 protons and 12 neutrons, what is its mass number?

<p>23 (A)</p> Signup and view all the answers

Which of the following is a homogeneous mixture?

<p>Saltwater. (C)</p> Signup and view all the answers

In standard atomic notation, where is the atomic number located?

<p>Bottom left (A)</p> Signup and view all the answers

What type of matter cannot be broken down into simpler substances by chemical means?

<p>Element (C)</p> Signup and view all the answers

Which of the following statements accurately describes the relationship between protons, neutrons, and electrons in an atom?

<p>Protons and neutrons are located in the nucleus, while electrons orbit around it. (D)</p> Signup and view all the answers

A student adds sugar to water and stirs until all the sugar disappears. In this scenario, what is the solvent?

<p>The water (D)</p> Signup and view all the answers

When reading a graduated cylinder, a student notices the water line is slightly curved. What is the name of this curve and where should the measurement be taken?

<p>Meniscus, bottom of the curve (D)</p> Signup and view all the answers

Flashcards

Inference

Conclusions or deductions based on observations.

Precipitate

Chemical reaction where a solid forms out of a liquid.

Density

The measure of how much mass is in a certain volume. Calculated as Mass/Volume.

Matter

Anything that takes up space and has mass.

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Volume

The amount of space something takes up.

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Subatomic particles

Tiny particles which are protons, electrons and neutrons.

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Periodic Table

A chart that organizes element by atomic number.

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Molecules

When atoms chemically combine.

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Mixture

A mixture where two or more substances are physically combined but not chemically.

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Interpolation

Assumption or prediction that the value is within the given time ranges.

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Study Notes

  • Inference involves conclusions or deductions based on observations.
  • GRASS represents Given, Required, Application, Solution, and Statement.
  • Precipitate refers to a chemical reaction where a solid forms out of a liquid.

Density

  • Defined as Mass(g) divided by Volume(^3).
  • Rounding is required.
  • For unit conversions, if there are two of the same units, putting one units alone and multiply one on the denominator (obv. w the numerator)
  • 1 cm^3 equals 1 mL.
  • To calculate mass, multiply, and for density and volume, divide.
  • Volume is calculated as D/M, Density as V/M, and Mass as VxD
  • Density measures how much mass occupies a certain volume.
  • Matter occupies space and has mass.
  • Volume is the amount of space something occupies.
  • All matter is made up of atoms.
  • Atoms are made up of subatomic particles: protons, electrons, and neutrons.

Periodic Table

  • Created by Dmitri Meldeeve.
  • Arranged by increasing atomic number.
  • Protons equal the atomic number.
  • Electrons are negative atomic number.
  • Neutrons are calculated by subtracting the atomic number from the mass number.
  • Mass number is at the top and the atomic number is at the bottom in standard atomic notation.
  • First 20 elements: H, He, Li, Be, B, C, N, O, F, Ne, Na, Mg, Al, Si, P, S, Cl, Ar, K, Ca.
  • Groups are arranged horizontally, comprising Alkali metals (first), Alkali earth metals (second), transition metals (3rd-12th), metalloids, halogens (17) and noble gases (18)
  • To count atoms, multiply numbers in brackets then add when beside the element
  • Molecules form when atoms chemically combine and exisit in air, molecules consist of Oxygen, Nitrogen, Water and carbon dioxide.
  • Families/Groups: Vertical columns where elements share similar chemical properties.
  • Energy shells are circles around the nucleus, with dots on the shells representing negative charge electrons and the nucles containing protons and neutrons
  • When writing atomic notation, atomic number is at the bottom, atomic mass is at the top, and the atomic number is the same as protons and electrons.
  • A heterogenous mixture contains easily distinguishable substances, like oil and water.
  • Homogenous mixtures are uniform, making individual substances indistinguishable, like milk.
  • A mixture involves two or more physically combined substances that are not chemically combined.
  • A pure substance contains only one type of molecule or atom and cannot be separated.
  • A solution is a mixture where everything is dissolved and appears uniform.
  • A mechanical mixture is similar to a heterogenous mixture, with visible and separable parts
  • Alloy: A mixture of two or more metals creating something stronger and useful.
  • Suspension: A mixture with floating bits that settle over time.
  • Elements cannot be broken down and contain only one type of atom.
  • Compound: A substance made from two different atoms that are joined.
  • Solute: What becomes dissolved.
  • Solvent: What dissolves the solute, exemplified by sugar being the solute and water/milk as the solvent.

Physical and Chemical Properties

  • Physical property: Measurable without changing the substance.
  • Chemical property: How a substance reacts when new substances are forms.
  • Physical change: Appearance changes, but the substance/chemical composition remain the same
  • Chemical change: A substance reacts and forms a new substance with different properties as chemical composition alters and changes
  • Physical changes are easily reversible, while chemical changes are not.

Unit Conversions

  • Only move the decimals
  • Kilo is the largest (1000), while milligram is the smallest (0.001).

Scientific Notation

  • For numbers > 10, move the decimal point to the left (positive), right before the last digit
  • For numbers < 1, move the decimal point to the right (negative), right before the last digit.
  • "The cause" is the independent variable
  • Independent variable: The one thing being changed in an experiment, usually by the experimenter, the x-axis on a graph
  • "Result of an experiment" is the dependent variable
  • Dependent variable refers to the result of the experiment, what is measured and what you changed as the y-axis on a graph.
  • Controlled Group: A group in an experiment that remains constant throughout the entire experiment and serves as a comparison for the experimental group.
  • Interpolation: Prediction or assumption of a value inside the time range
  • Extrapolation: Prediction or assumption of a value outside of the time range
  • Quantitative observations are measurable or countable data.
  • Qualitative observations are descriptive, not numerical.

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