Master this deck with 126 terms through effective study methods.
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A phenomenon is an observable event or occurrence. An example is the process of photosynthesis in plants.
They provide a framework for understanding the natural world, allowing scientists to make predictions and establish reliable theories.
Scientists observe, experiment, and analyze data to understand natural phenomena and develop theories.
SI stands for the International System of Units, which is a standardized system of measurement used in science.
It states that every effect has a specific cause, which is fundamental in scientific inquiry.
It asserts that the laws of nature are consistent over time and space.
1. Ask a question 2. Conduct background research 3. Formulate a hypothesis 4. Test the hypothesis by conducting experiments 5. Analyze data and draw conclusions 6. Communicate results 7. Repeat the process if necessary 8. Develop a theory.
Physical models, conceptual models, and mathematical models.
By exploring, understanding, and stewarding the natural world as a reflection of God's creation.
The three foundations are Scripture, Tradition, and Reason.
What does the Bible say about this issue?
What are the results of following biblical principles?
What are the underlying motivations for actions according to biblical teachings?
Qualitative data describes characteristics or qualities, while quantitative data involves numerical measurements.
Laws describe observable phenomena consistently, while theories explain the underlying reasons for those phenomena.
The directive given by God to humanity to fill the earth and steward creation.
A globe representing the Earth.
The atomic model illustrating the structure of an atom.
The equation for calculating the trajectory of a projectile.
The arrangement of leaves on a stem and the periodic table of elements.
Naturalism and theism.
Descriptive models and predictive models.
1. Meter (m) - length 2. Kilogram (kg) - mass 3. Second (s) - time 4. Ampere (A) - electric current 5. Kelvin (K) - temperature 6. Mole (mol) - amount of substance 7. Candela (cd) - luminous intensity.
Derived units are combinations of SI base units. An example is the unit of force, the Newton (N), which is kg·m/s².
Wafting is a technique used to safely smell a substance by gently waving the air towards your nose.
Physics and chemistry.
Qualitative data.
The fourth step: Test the hypothesis by conducting experiments.
The second step: Conduct background research.
(This requires visual input and cannot be answered without images.)
Matter is anything that has mass and occupies space.
False. Matter does not include light, sound, and warmth as they do not have mass.
1. Brownian motion 2. Gases exerting pressure 3. The behavior of solids, liquids, and gases.
The Kinetic Molecular Theory.
Particles are the small constituents that make up matter, including atoms and molecules.
Atoms are the basic units of matter, while molecules are formed when two or more atoms bond together.
Density (d) = mass (m) / volume (V).
Mass (m) = density (d) × volume (V).
Volume (V) = mass (m) / density (d).
Weight is the force exerted by gravity on an object, calculated as mass times the acceleration due to gravity.
Pure substances and mixtures.
Elements and compounds.
Compound.
Element.
Homogeneous mixtures and heterogeneous mixtures.
Salad and sand mixed with iron filings.
Saltwater and air.
Solid, liquid, gas, and plasma.
Energy of motion.
Solid.
Plasma.
Liquids and gases.
Gas.
To organize and understand the natural world.
Liquid.
A characteristic of matter that can be observed or measured without changing its identity.
Color, density, melting point, boiling point, solubility, and conductivity.
A characteristic of a substance that describes its ability to undergo a specific chemical change.
Reactivity with acids and flammability.
Matter cannot be created or destroyed in a chemical reaction.
Chemical change.
Physical change.
Chemical change.
Physical change.
Chemical reaction.
Density = mass/volume.
Density = 72 g / 9 mL = 8 g/mL.
Mass = density × volume.
Mass = 2 g/mL × 5 mL = 10 grams.
Volume = mass / density.
Volume = 360 g / 60 g/mL = 6 mL.
(This requires visual input and cannot be answered without images.)
It explained the repulsion and deflection of alpha particles by the positively charged nucleus.
Workability is the ability of a material to be shaped or molded without breaking.
Gold, silver, iron, copper, lead, tin, and mercury.
Earth, water, air, fire, and aether.
Opposite charges attract and like charges repel.
The Quantum Mechanical Model.
Because it provides a simple way to visualize electron arrangements.
(This requires visual input and cannot be answered without images.)
The neutron was discovered in 1932 by James Chadwick.
Because neutrons are neutral and do not produce electric charge effects, making them harder to detect.
Protons and neutrons.
Electrons.
Gold's atomic number is 79, and its atomic mass is approximately 197 u.
An isotope is a variant of a chemical element that has the same number of protons but a different number of neutrons.
The mass number is the total number of protons and neutrons in an atom's nucleus.
Isotope notation represents an isotope's mass number and atomic number. The general form is A/Z Element, where A is the mass number and Z is the atomic number.
The isotope notation for sodium-23 is 23/11 Na.
Ions are charged particles that result from the loss or gain of electrons.
Cations.
Anions.
Atomic mass is the weighted average mass of an element's isotopes, expressed in atomic mass units (u). It is usually a decimal because it accounts for the relative abundance of each isotope.
The atomic number is the number of protons in an atom, while the atomic mass is the average mass of an atom, including protons and neutrons.
1. Most alpha particles passed through the foil. 2. Some alpha particles were deflected at small angles. 3. A few alpha particles were deflected back at large angles. 4. The atom is mostly empty space. 5. There is a small, dense, positively charged nucleus.
Protons.
Electrons.
Neutrons.
A chemical bond.
The Octet Rule states that atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration.
Cations.
Anions are ions that have gained electrons and have a negative charge.
Electronegativity is the tendency of an atom to attract electrons in a chemical bond.
A covalent bond is a chemical bond formed when two atoms share one or more pairs of electrons.
A diatomic molecule consists of two atoms of the same or different elements bonded together.
Lewis structures are diagrams that represent the bonding between atoms and the lone pairs of electrons in a molecule.
A single covalent bond is formed when two atoms share one pair of electrons.
A triple covalent bond is formed when two atoms share three pairs of electrons.
A polar covalent bond is a type of bond where electrons are shared unequally between atoms, resulting in a dipole moment.
A nonpolar covalent bond is a type of bond where electrons are shared equally between atoms.
Useful energy.
Atoms form chemical bonds to achieve stability by filling their outer electron shells.
Stable.
Their electron configurations.
Eight.
By gaining electrons to form anions or losing electrons to form cations.
1. Water is a liquid at room temperature, while hydrogen and oxygen are gases. 2. Water has a high specific heat capacity, which is not a property of hydrogen or oxygen.
Eight; losing.
Nonmetals.
Metals and nonmetals.
Metal atoms.
Gilbert N. Lewis.
Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Bromine (Br2), and Iodine (I2).
Triple covalent bonds are stronger.
Ionic bonds form between atoms with dissimilar electronegativities, and the atoms transfer electrons. An example is sodium chloride (NaCl).
Salts are formed through ionic bonds between metals and nonmetals. Examples include sodium chloride (NaCl), magnesium oxide (MgO), and calcium fluoride (CaF2).