Chemistry- Unit 1: Atomic Properties

a region in an atom where there is a high probability of finding electrons

a region of an atom in which electrons of the same energy are likely to be found

2 electrons in orbital

6 electrons in orbital

10 electrons in orbital

14 electrons in orbital

18 electrons in orbital

no two electrons in the same atom can have the same set of four quantum numbers

The lowest energy state of an atom

A state in which an atom has more energy than it does at its ground state, going to a higher energy level

G: 1s^2 2s^2 2p^3 E:1s^2 2s^2 2p^2 3s^1

An electron occupies the lowest-energy orbital that can receive it

single occupancy of orbital before pairing

An atomic orbital may describe at most two electrons, each with opposite spin direction

Electrons on the outermost energy level of an atom

electrons in the energy levels between the nucleus and the valence electrons

size of an atom

increases down a group, decreases across a period

down because of more energy levels meaning more shielding electrons

across because of effective nuclear charge increases

The energy required to the remove an electron from the outer shell of an atom.

increases up and to the right

the ability of an atom to attract electrons when the atom is in a compound

increases up and to the right

the energy required to remove the first electron from an atom

The outer electrons are further away from the nucleus and hence are not as tightly held

effective nuclear charge increases as electron shielding remains constant, so it is harder to take the electron

The outer electrons are further away from the nucleus and hence are not as tightly held

effective nuclear charge increases as electron shielding remains constant, so it is harder to take the electron

+2

must use roman numerals

A negatively charged ion

A positively charged ion

A rule that states that an atom will give up, accept, or share electrons in order to achieve a filled outer electron shell, which usually consists of 8 electrons.

A charged group of covalently bonded atoms

two or more atoms held together by covalent bonds

A mixture of two or more metals

pair of electrons not invovled in bonding instead by exclusively a single atom

stable and exothermic

unstable and endothermic

Formed when one or more electrons are transferred from one atom to anothe

cations (metal) to anions (salt)

high melting points, good solubility in water, poor conductors of heat and electricity in lattice and brittle

repeating pattern of positive and negative ions forming an ionic compound

Describes a force between particles with opposite electrical charges that causes them to push apart from one another

the attraction between positive and negative charges

a type of covalent bond between atoms that differ in electronegativity. the shared electrons are pulled closer to the more electronegative atom. making one slightly negative and the other slightly positive

Bonds created by sharing electrons with other atoms.

the sharing of two pairs of electrons between two atoms

a type of bond that forms when electrons are not shared equally

a covalent bond in which one atom contributes both bonding electrons

atoms covalently bonded into a large structure that does not contain a specific number of atoms

-share electrons -lower melting point -lower boiling point -poor conductors

very hard, very high melting points, poor conductors

a bond formed by the attraction between positively charged metal ions and the electrons around them

electrons that are free to move in metals

good heat and electricity conductors in both molten and solid state, ductile, malleable, luster, high melting and boiling point

light being reflected of movement of valence electrons

A charged group of covalently bonded atoms

can measure the number of electrons in an area

Sum of (isotope abundance x isotope mass number) / 100

onyl has single bonds

double or more bonds

The study of the properties of light that depend on wavelength.

both a particle and a wave

particles of light energy that are completely weightless

Testing chemicals by burning a compound to look at its flame color. Certain compounds and elements burn with distinctive colors.

Yellow flame

Lilac flame

Crimson flame

Green flame

Orange-red flame

a device that spreads light into its different colors

pigments absorb certain colours of light by an atom when electrons get excited by certain wavelengths and move up energy levels, the remaining colours of light are reflected

excited electron going back down to a grounded state giving out light energy as it returns down

the mass relative tot he space an object takes up