Aleks Placement Test: Chemistry Part 1

Anything that has mass and takes up space; made of atoms

Basic unit of matter which cannot be broken down and contain mostly empty space; contains three parts: the electron, proton, and neutron

A pure substance that contains only one type of atom

Two or more elements that are chemically bonded; includes ionic and covalent

Two or more substances that are together but not bonded

Substance that contains only one kind of compound

The state of matter with the lowest energy; basically a very cold solid

A state of matter with strong bonds

A state of matter with weak bonds

A state of matter with no bonds

The state of matter with the highest energy; it uses ionization instead of bonds

First to define an element; any substance is a substance unless it can be broken down

Used and combined previous ideas to discuss the atom; elements are made of atoms; all atoms of an element are identical; atoms of different elements are different; law of constant composition; atoms are invisible

Atoms of one element can combine with other elements to form compounds; a given compound always has the same relative numbers and types of atoms

Discovered electrons and protons and developed the plum pudding model of an atom

The negatively charged particle in an atom; circles around the nucleus in the electron cloud

The positively charged particle in an atom; located in the nucleus; determine the element

The neutral particle in an atom; it has no charge and is located in the nucleus

A model of the atom that depicts a sphere of positive charge with electrons scattered throughout

Conducted an experiment in which he shot alpha particles at gold foil; roved there was a small, dense nucleus with a positive charge and that protons are positive

Elements located on the left side of the periodic table that want to lose electrons

- Malleable

- Ductile

- Conductive

- Lustrous

The ability to be molded into shapes

The ability to be pulled into wire

The ability to allow heat or electricity to pass through an object

The ability to be shiny

Elements located on the right side of the periodic table that want to gain electrons

Elements placed in a stair-step line between metals and nonmetals; they have characteristics of both

Elements that occur in pairs in their natural state; hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

The ability of a molecule to attract electrons to it; increases as you move left to right in the table and decreases as you move top to bottom; fluorine is the hardest

The radius of an atom; decreases as you move left to right and increases as you move top to bottom

The energy needed to rip off an electron; increases as you move left to right and decreases as you move top to bottom

An atom that has gained or lost electrons

An atom that gains electrons and has a negative charge; nonmetals

An atom that looses electrons and has a positive charge; metals

An atom that has changed its number of neutrons

A unique number to each element that tells the number of protons and the number of electrons if the atom is neutral

A number that tells the number of protons and neutrons in an atom

Atomic Mass - Atomic Number

A nucleus that spontaneously decomposes, forming a different nucleus and producing one or more particles; alpha, beta, and gamma ray

One type of radioactive particle; it is a essentially a helium nucleus; when this type of particle is released, the mass of the atom is conserved and so is the atomic number

One type of radioactive particle; it is essentially an electron; when this type of particle is released, the atomic mass is conserved and the atomic number gains one (a neutron is changed to a proton)

One type of radioactive particle; it is a high energy photon of light and is used to release excess energy; the atom is not changed at all

The time required for half of the original sample of nuclei to decay; each radioactive nucleus of the same element has the same half-life; the shorter the half-life, the more likely a nucleus will decay

Elements exist naturally in different isotopes, to the atomic mass listed on the table is an average

Average Mass = (%)•(Mass of Isotope A) + (%)•(Mass of Isotope B) +...

The highest point of a wave

The lowest point of a wave

The distance between the crests of a wave; symbol is lambda

The number of waves that pass through a point in a given time; symbol is nu

The height of a crest or trough; crest to the zero line; absolute value

How fast a wave travels in a given distance

Point on a wave where the wave returns to the zero line; a crest or trough is trapped between the two points

The range of wavelengths or frequencies over which electromagnetic radiation extend

White light is passed through a prism and creates all visible colors; each color has its own frequency and wavelength

When an atom is excited by energy it gives off its own characteristic colors of light

A light particle

C = w•f

C is the speed of light

w is wavelength in meters

f is frequency in hertz

3.00•10^8m/s

Broken bands of colored light

a.k.a. emission spectrum; occurs due to the energy an electron gives off as it travels from high to low energy; fireworks

a.k.a. absorption spectrum; occurs due to the energy that an electron gains as it travels from low to high energy

E = h•f

E is energy

h is Planck's constant

f is frequency in hertz

6.626•10^-34 Joules/hertz

Light sometimes acts like a particle and sometimes like a wave

A model of the atom in which the orbitals are nothing like orbits

It is impossible to know the exact position and momentum of an electron at the same time

The probability of finding electrons in certain regions of an atom is described by orbitals

A region around the nucleus of an atom where an electron with a given energy may be found 90% of the time; 4 types: s, p, d, and f

The principal quantum number; tells us which energy level an electron is found in, the maximum number of electrons that can be found in one energy level, and the size of an electron cloud

The orbital quantum number; tells us the shape of the orbital (s,p,d,f)

Quantum number that tells us the orientation of the orbital in space

Quantum number that tells how an electron spins in an orbital

A rule that states that each electron has its own unique set of quantum numbers and that two electrons with the same spin cannot occupy the same orbital and that an orbital can only hold two electrons

The orbital with the lowest energy; it has one orbital and can hold two electrons

The orbital with the second lowest energy; it has three orbitals and can hold six electrons

The orbital with the second highest energy; it has five orbitals and can hold ten electrons

The orbital with the highest energy; it has seven orbitals and can hold 14 electrons

Each suborbital will fill with one electron before accepting a second electron

Electron configuration shorthand

1. Find the noble gas that comes before the element

2. Write the gas in brackets

3. Determine energy level and orbital you are starting on

4. Follow the energy pyramid

Electrons on outer most orbital; always the highest energy 's' and 'p' orbital

The electrons an element will gain or lose in order to become stable (8 electrons)

Always start with hydrogen; donate a proton in a solution

Acid that has an oxygen

Acid that contains a carbon atom

Acid that has 2 hydrogens to donate

Acid that has 3 hydrogens to give

______ic acid

_______ous acid

1 carbon

2 carbon

3 carbon

4 carbon

5 carbon

6 carbon

7 carbon

8 carbon

9 carbon

10 carbon

Subtract a hydrogen and add a -OH group; add ol to end of name