chemistry

Atoms

the fundamental building blocks of matter and life

Elements

the simplest form of matter that has a characteristic set of properties

Molecules

2 or more elements combined to form a structure

Energy

the capacity to move, do work, change matter, or produce heat

Kinetic Energy

the energy that matter has because of its motion

Thermal Energy

refers to the energy contained within a system that is responsible for its temperature

Potential Energy

the stored energy in matter due to its position relative to other matter

chemical potential energy

the energy stored in the chemical bonds that hold atoms together

Macroscopic properties

a characteristic that is large enough to see handle or measure without magnification

subatomic particles

protons, neutrons and electrons

Proton

the subatomic particle with a positive charge

neutron

the subatomic particle with a neutral charge

electron

The subatomic particle with a negative charge

Nucleus

The central part of an atom which is made up of protons and neutrons

Atomic Number

number of protons in an atom

Mass Number

the sum of protons and neutrons

isotopes

Elements that have the same proton number, but different neutron number

Atomic mass

The mass of a single atom

proton mass

1.67 x 10⁻²⁴ grams / 1+ amu

neutron mass

1.67 x 10⁻²⁴ grams/ 1 amu

electron mass

9.11 x 10⁻²⁸ grams/ 0.0005 amu

Atomic Emission Spectra

The pattern formed when light emitted by an element is separated into different wavelengths it contains

Bohr Model

An atomic model that described electrons as moving in circular orbits around the nucleus

quantum of energy

The amount of energy needed to move an electron from one level to another

Q) 1: what distinguishes the colors of a mountain?

Unique colors of a mountain is due to the different minerals that have been exposed and oxidized over a long time. different minerals, like sandstone, limestone, and iron oxide in the mountain contribute distinct colors like red, green and white.

Q) 2: what does distinguishes the colors of a firework?

Through the phenomenon of incandescence and luminesence. The materials inside different wavelength to light. Each wavelength corresponds to a different color. E.g. Sodium gives yellow lights in a flame.

Incandescence.

Heating a metal until it shines white.

luminescence.

Heating of a metal (powdered form) until it produces a color

Q5) density is the matter in a given volume. Materials that are less dense on denser materials. Use the models to explain, on a molecular level, white ice floats on water. (use ur textbook for help)

density is a measure of how crammed together molecules are. More dense objects have more molecules crammed together in a smaller space. Less dense objects tend to float on denser liquid liquids. Sunset floats on water, it's less dense. however, in most cases, the solid form of a substance is generally more dense than its liquid form. H2O is an exception.

Q7) liquid gallium changes to gas at 2229°C. Describe how a model of gases gallium would compare to the model of liquid gallium shown in the picture.. (use ur textbook to help u)

Liquid gallium flows into different shapes, but its volume does not change. The particles in liquid gallium have more kinetic energy than those solid gallium, but less than the particles in gaseous gallium.

What atom are Diamond and Coal made up of?

Carbon

Q11) based on the organization and colors in the periodic table, which two elements do you think the most similar in terms of their properties. Magnesium (Mg), barium (Ba), and gold (Au)? Explain.

Magnesium and barium would have similar properties since they are located above and below each other.

Q13) how does the overall charge of oxygen-16 compared to the overall charge of oxygen-17 and oxygen-18? use the models of isotopes to help explain your answer. (Use your textbook to help u)

Charge does not change among isotopes because the number of protons is the same as the number of electrons. All are electrically neutral.

Q15) Look at the graphs. How does an elements atomic mass compared to the mass number of its most abundant isotope?

Generally, the atomic mass of an element is the same whole number as the mass number of its most common isotope.

Formulae of atomic mass

[Mass number of Isotope 1 × 1%] + [Mass number of Isotope 2 × 2%]

Q17) in what ways are final grade calculations and atomic mass calculations similar?

Final grade at atomic mass calculations are similar because both use the concept of a weighted average to determine a final value.

Q19) how does an elements atomic mass differ from its mass number?

Mass number is the total number of protons and neutrons in the nucleus of an element. Whereas, atomic mass is the average of mass number of all isotopes of the element. Atomic mass (Not mass number) it's more often used in calculations.

Q21) what is the identity of the element that produced the unknown emission spectrum and what information does the spectrum give about the source of the element?

Stranium is the unknown element. The emission spectrum of the unknown element is identical to that of Stranium.