Chemistry 1101 Final Exam Review

Flashcards for Chemistry 1101 Final Exam Review

Matter

The physical material of the Universe; anything that has mass and takes up space.

Elements

Elementary substances that which all matter can be broken down into.

Homogenous Mixture

A mix of substances that cannot be easily separated.

Heterogenous Mixture

A mix of substances that can be easily separated. (e.g., A Salad)

Intensive Property

Any property of matter that does not depend on the amount of matter present. E.g. Density.

Extensive Property

Any property of matter that does depend on the amount of matter present. Eg. Mass

Density

The amount of mass per unit Volume.

SI units

Standard units that we will use for measurement.

Significant Figures

Number of digits to reflect the accuracy of measurement and the precision of the measuring device.

Rule of Significant Figures: Non-Zero Numbers

All non-zero numbers are significant.

Rule of Significant Figures: Zeros Between Digits

Zeros between digits are significant.

Rule of Significant Figures: Leading Zeros

Zeros at the beginning of a digit are not significant.

Rule of Significant Figures: Trailing Zeros after Decimal

Zeros at the end of a number and after a decimal point are significant.

Rule of Significant Figures: Trailing Zeros without Decimal

When a number has no decimal point but the number has trailing Zeros, they aren't significant.

Dimensional Analysis

A usefull tool to help keep units in Check.

Dalton's Atomic Theory - Postulate 1

Each element is comprised of small things called atoms.

Dalton's Atomic Theory - Postulate 2

Atoms of a given element are identical, but atoms of one element are different from one another.

Dalton's Atomic Theory - Postulate 3

Atoms of one element cannot change into a different element in chemical reactions.

Dalton's Atomic Theory - Postulate 4

Compounds are formed when two or more elements react together.

The Electron

Discovered by J.J Thomson (1897)

Earnest Rutherford's Gold Foil experiment

Showed that the atom has a central nucleous and space between them.

Proton

Positive charge in the nucleus

Neutron

No charge in the nucleus

Electron

Negative Charge outside the nucleus

Atomic Number

Notation of figuring out which atom is which

Isotopes

Atoms with same number of protons but different number of neutrons.

The periodic table

Table of elements that tells us properties of the elements we percieve

Cations

Formed when the atom loses an electron

Anions

Formed when an atom gains an electron

Ionic Compounds

Metal and non-metal bound together. No prefix needed when naming. On the Anion, the Suffix ide is added. When writing the order is Cation; Anion. The subscript is based of charge of the atoms.

Covalent Compounds

Two or more non-metals bind together is called a Covalent bond, We use prefixes such as, mono, di, tri ect. Also use the suffix ide. If its only one on the first element, we do not use mono prefix

Metalic Naming

We denote the charge of the metal with a roman numeral and Use Ionic naming

Properties of Light

Light as we know it is Electro magnetic Radiation.

Frequency

Tells us how many cycles, or wavelengths per second. In units of /sec

Quantization of Energy

Light is quantized in discrete energy packets

The photoelectric Effect

Amount of energy a wave of electromagnetic need to have to strike metal in which an electron is released.

The Bohr model

Anucleus at the center with different discrete energy levels

Key idea of Bohr Model

Electrons exist in discrete energy levels and Energy is involved in moving an electron from one energy level to another,

de Broglie wavelength

The mass of the wave

Electron Pair

Pair of electrons with opposite spins (↑↓)

Types of Electrons

Spin up (↑) and a spin down (↓) electron.

S-Orbital

Can only hold up to 1 electron pain (2e- total)

P- Orbital

Can hold up to 3 electron pairs (6e- total)

D-orbital

Can hold up to 5 electron pairs (10e- total)

f-orbital

Can hold up to 7 electron pairs (14e- total)

Pauli Exclusion principal

The property of electron pains being One Spin up and one spin down. The arrows signify the order in which the electrons fill the shells/orbitals.

Hund's Rule

Spin up electrons fill orbitals before spin down electrons, keep this in mind when writing electron configurations.

Effective Nuclear Charge

The Charge the nucleus feels from its electrons

Ionization Energy

The minimum energy required to remove an electron from the ground state of an atom.

Electron Affinity

The energy change when an electron is added to an atom.

Electronegativity

The tendancy to attract electrons when forming a bond.

Conservation of Mass

In a reaction the stuff going in must equal the stuff coming out.

Combination Reaction

A+B->C

Decomposition Reaction

C->A+B

Combustion Reaction

fuel + O2 -> H₂O + CO₂

Avogadros Number

Molar mass

Limiting Reactants

If we have a reaction with 2 or more reactants, we need enough ingredients to make something right? but if we dont we do our stoiciometric calculation and take the lowest mass.

Molarity

known as Concentration.

The octet rule

Atoms normally are happy with 8 valence electrons, Like the noble gases.

Ionic bands

A metal and non-metal come together where the Anion "Takes" the Cations V.E. to fill its shell. This is only an electrostatic Interaction

Covalent Bonds

The atoms 'share' the electrons to fill each others shells

Hybridization

Steric Number: number of sigma bonding electrons + number of non-binding electrons