Chemistry MIDTERM Study Guide

there is no way this works out for me

atomic number

Elements on modern periodic table are arranged in order of increasing _____________

Period

horizontal row, numbered 1-7 (except for f-block)

Group or Family

vertical columns, numbered 1-18

Inner transition metals

f-block, lanthanide series and actinide series

Main group or Representative elements

elements in tall columns (s- and p-blocks)

properties

Modern periodic table is based on _____________

Transition elements

d-block and f-block

Metals

gray/silver, shiny, malleable, ductile, good conductors, solids (left of the stair step line)

Alkaline earth metals

group 2

Properties

behaviors or characteristics

Transition metals

groups 3-12, d-block

Bromine

_____________ is a nonmetal liquid

Lanthanide series

elements 57-71

Nonmetals

variety of colors, gasses, brittle, dull-looking solids, insulators, poor conductors of electricity and heat, located to the right of the stair step line (includes hydrogen)

similar valence electrons

Elements in groups have the same properties because they have _____________

Alkali metals

group 1 (excluding hydrogen), reactive

Magnesium and Calcium

_____________ and _____________ compounds are important nutrients for people

Atomic radius

the distance from the center of the nucleus to the most probable location of the outermost valence electron in an atom, unit is picometer

Oxygen

_____________ is the most abundant element in the human body

Halogens

group 17, usually found as parts of compounds

fluorine

Compounds of _____________ are used to prevent tooth decay

Noble gases

group 18, unreactive, used in lasers, light bulbs, and neon signs

Metalloids

properties of both metals and nonmetals, used in computer chips and solar cells

the same number of valence electrons

Atoms in the same group have similar chemical properties because they have _____________

Ionization energy

required to remove an electron from one mole of a gaseous substance

electron configurations

Element properties come from their _____________

Ions

charged particles formed when an atom or a group of atoms loses or gains electrons

Actinide series

elements 89-103

Cations

positively charged ions formed by losing electrons, smaller than their neutral atoms, largest ionic radii are at the bottom left (metals)

Anions

negatively charged ions formed by gaining electrons, larger than their neutral atoms, largest ionic radii are at the bottom left (nonmetals)

Mercury

_____________ is a silver-colored, metal liquid

stable

Ions are made to form more _____________ electron configurations

bottom left

Atomic radii are greatest toward the _____________

Ionic radius

the distance from the center of the nucleus to the most probable location of the outermost valence electron in an ion, unit is picometer

Low electronegativity

little attraction for electron in bond

First ionization energy

the energy required to remove the most loosely bound electron (outermost valence electron) from a gaseous atom, turning it into a cation with a 1+ charge, symbol: I1 or IE1, unit: kJ/mol

Ionization energy is low

electron is easily removed

Ionization energy is high

electron is difficult to remove

top right

First ionization energies are greatest toward the _____________

Electronegativity

the relative tendency of an atom to attract the electrons involved in a chemical bond with another atom, unit-less number ranging from 0-4, greatest values are toward top right, not defined for noble gases

High electronegativity

strong attraction for electron in bond

Octet rule

states that atoms tend to gain, lose, or share electrons until they achieve a stable electron configuration, usually one with 8 valence electrons or a full valence shell of electrons

Chemistry

the study of matter and the changes it undergoes

Matter

anything that has mass and takes up space

Pure substance

matter that has a definite composition, a chemical formula

Element

pure substances that cannot be broken down into simpler substances by physical or chemical means

Atom

the smallest particle of an element that retains all the properties of the element

Modern Atomic Theory

All matter is composed of small, divisible particles called atoms. Not all atoms of the same element are identical (isotopes). Atoms of different elements are different. Atoms can bond with one another in simple ratios to form compounds.

Subatomic particles

particles smaller than atoms (proton, neutron, electron)

Atomic mass unit

unit of mass for expressing masses of atoms or molecules; 1/12 of the mass of an atom of carbon-12

Nucleus

located in the center of the atom, small in volume, positively charged, contains most of the atom's mass

Electrostatic attraction

the attraction between oppositely charged particles (negative electrons to positive protons)

Electron

symbol: e-, charge: 1-, mass: 0 amu, location: empty space around nucleus/ electron cloud

Proton

symbol: p+, charge: 1+, mass: 1 amu, location: nucleus

Neutron

symbol: n0, charge: 0, mass: 1 amu, location: nucleus

Atomic number

the number of protons in an atom, symbol: Z, whole number located in the box, makes an element a particular element.

Isotopes

atoms with the same number of protons, but different numbers of neutrons, same element that differ in mass number

Mass number

the sum of the number of neutrons and protons in an atomic nucleus, symbol: A, NOT on most periodic tables

Atomic mass

the weighted average mass of the naturally occurring isotopes of an element, (%)(mass) + (%)(mass) + ...

Radioactivity

the spontaneous emission of radiation

Radiation

energy rays and/or particles

Radioactive decay

to fall apart by giving off nuclear radiation, until they become stable

Ratio of neutrons to protons

what determines the stability of an atomic nucleus

Nuclear reaction

the atom's nucleus changes, often turns into a different element

Nuclear equation

symbolizes a nuclear reaction

Alpha radiation

helium-4, consisting of 2 protons and 2 neutrons, mass: 4 amu, charge: 2+

Beta radiation

a high-speed electron emitted from a radioactive nucleus, mass: 0 amu, charge: 1-

Gamma radiation

a high-energy form of electromagnetic radiation, has no mass and no charge, not a particle, just energy

Fission

a neutron slams into a larger atom, forcing it to split into two smaller atoms (splits)

Fusion

two atoms slam together to form a heavier atom (fuse)

Law of Conservation of Mass-Energy

mass and energy can be converted from one to the other, but their sum remains constant

Circle graph

shows the parts of a whole/ percentages

Bar graph

evaluates trends in a measured property often as a function of time, location, or temperature

Line graph

determines property trend or the mathematical relationship between two variables

Direct relation

positive slope, straight line

Indirect relation

negative slope, straight line

Inverse relation

hyperbola, a curve with a negative slope that never crosses an axis

Electromagnetic radiation

a form of energy that exhibits wavelike behavior as it travels through space

Wavelength

the shortest distance between 2 equivalent points on a continuous wave

Units for wavelength

meter or nanometer

Symbol for wavelength

lambda, λ

Frequency

the number of waves that pass a given point per second

Unit for frequency

hertz, 1/s

Symbol for frequency

nu, ν

Amplitude

the wave's height from the origin to a crest or trough

Speed of light equation

c (speed of light, m/s) = λ (wavelength, m or nm) * ν (frequency, hertz)

inversely

Wavelength and frequency vary ________.

Electromagnetic spectrum

a spectrum that includes all forms of electromagnetic radiation

Quantum theory

a theory created by Max Planck to explain how matter lost and gained only small, specific amounts of energy

Quantum

the minimum amount of energy that can be lost or gained or gained by an atom

Photon

a particle-like bundle of energy without mass that carries a quantum of electromagnetic energy

Energy of a photon equation

E (energy, joules) = h (Planck's constant, joules * seconds) * ν (frequency, hertz)

Spectroscopy

the method of studying substances exposed to energy

Spectrum

the pattern of energy studied in spectroscopy

Atomic emission spectrum

the set of frequencies or wavelengths of the electromagnetic waves emitted by atoms of the element

unique

Each element produces a ________ line spectrum.

Bohr's (planetary) model

an early atomic model of the hydrogen atom that was developed by studying the emission spectrum of hydrogen

Accurate part of Bohr's model

the electron can only posses certain quantities of energy/ have certain allowed energy states

Ground state

the lowest and most stable energy state

Excited state

any state of energy that is more than the lowest amount