Answer: Because milk has higher KE than ice, KE is transferred from the milk to the molecules of ice.
Answer: a suspension
Answer: 3.47 x 10^24
Answer: Na = 27.36%, H = 1.20%, C = 14.30%, O = 57.14%
Answer: C6H12O6
Answer: 48.83%
Answer: 74.02%
Answer: C2H6
Answer: Halogens tend to gain one electron so that they can get a full outer level and be stable.
Answer: Because most of them have 3 or less valence electrons.
Answer: Metals tend to lose electrons and nonmetals tend to gain electrons.
Answer: It is a metal because it it only has two valence (outer level) electrons. Metals tend to have 3 or less valence electrons.
Answer: Metals are shiny, malleable and good conductors whereas nonmetals are dull, brittle, and insulators.
Answer: No
Answer: Yes
Answer: Yes
Answer: Solid
Answer: High
Answer: No
Answer: No apart from graphite which does
Answer: Solid
Answer: High
Answer: Depends on the polarity of the molecule
Answer: No
Answer: No
Answer: May be solid (I2) but usually liquid or gas
Answer: Low
Answer: Yes
Answer: Yes
Answer: No
Answer: Solid
Answer: High
The melting and boiling points of a substance are determined by the strength of the attraction between its particles
A substance will only conduct electricity if it contains charged particles that are free to move
How soluble a substance is in water depends on the particles it contains, water is a polar solvent, so charged or polar substances will dissolve in it well while others will not
Answer: To melt or boil a simple covalent structure you don't have to overcome the the strong covalent bonds that hold the atoms together in the molecule, you only have to overcome the intermolecular forces between molecules which are much weaker
Answer: In gases the particles have loads more energy and are much further apart, so the density is pretty low and it's very compressible. The particles move about freely with not a lot of attraction between them so they'll quickly diffuse to fill a container
A typical liquid has a similar density to a solid and is virtually incompressible
The particles move about freely and randomly within the liquid allowing it to flow
A solid has its particles very close together giving it a high density and making it incompressible
The particles vibrate around a fixed point and can't move about freely
Answer: Bc of the strength of the metallic bonds
Answer: The delocalised electrons can move and carry charge
Answer: The delocalised electrons can pass kinetic energy to each other
The more delocalised electrons per atom the stronger the bonding will be and the higher the melting point eg Mg2+ has a higher melting point than Na+
Answer: Strong electrostatic forces of attraction between the positive metal ions and the delocalised sea of electrons
High melting points
Good thermal conductors
Good electrical conductors
Insoluble
The outermost shell of electrons of a metal atom is delocalised leaving a positive metal ion
The positive metal ions are attracted to the delocalised negative electrons forming a lattice of positive ions electrostatically attracted to the oppositely charged sea of delocalised electrons
Answer: As giant metallic lattice structures
As liquid water cools to form ice, the molecules make more hydrogen bonds and arrange themselves into a regular lattice structure.
In this structure the H2O molecules are further apart on average that the molecules in liquid water so ice is less dense than liquid water
Answer: Bc of the extra energy needed to break the hydrogen bonds
Answer: Fluorine, Nitrogen and Oxygen are very electronegative, so they draw bonding electrons away from the hydrogen atom. The bond is so polarised, and hydrogen has such a high charge density (bc it's so small) that the hydrogen atoms form weak bonds with lone pairs of electrons on the fluorine, nitrogen and oxygen atoms of other molecules
Answer: when there is an H that can bond to N, O, or F
Answer: Long straight molecules can lie closer together than branched ones, and the closer two molecules are to each other the stronger the intermolecular forces between them
Answer: Larger molecules have larger electron clouds meaning stronger VDW
Electrons in charge clouds are always moving really quickly and at any moment they are more likely to be more to one side of an atom than the other. At this moment, the atom would have a temporary dipole
This dipole can cause another temporary dipole in the opposite direction on a neighbouring atom. The two dipoles are then attracted to each other.
The second dipole can cause another dipole in a third atom like a domino effect.
Bc electrons are constantly moving, the dipoles are being created and destroyed all the time. Even though the dipoles keep changing, the overall effect is for the atoms to be attracted to each another
Answer: Forces found between all atoms and molecules causing them to be attracted to each other
Answer: They affect the physical properties of a compounds
Van der Waals
Permanent dipole-dipole
Hydrogen bonding
Answer: Permanent dipoles which are weak forces of electrostatic attraction between the §+ and §- charges on neighbouring molecules
Answer: The charges cancel out bc they are opposite each other eg CO2
Answer: When there is an uneven distribution of charge across the whole molecule eg water
Answer: A difference in charge between two atoms in a polar bond caused by a shift in electron density in the bond
Answer: An atoms ability to attract the electron pair in a covalent bond
6 bonding
0 lone
90©️
90©️
5 bonding
1 lone
90©️
5 bonding
0 lone
90©️
4 bonding
2 lone
90©️
4 bonding
1 lone
102©️
87©️
4 bonding
0 lone
109.5©️
3 bonding
2 lone
88©️
3 bonding
1 lone
107©️
3 bonding
0 lone
120©️
2 bonding
2 lone
104.5©️
2 bonding
0 lone
180©️
Answer: Valence-Shell Electron-Pair Repulsion Theory
Lone pair / Lone pair
Lone pair / Bonding pair
Bonding pair / Bonding pair
Answer: Electrons are all negatively charged so the charge clouds will repel each other as much as they can so the pairs of electrons in the outer shell of an atom will sit as far apart as they possibly can
Answer: An area where you have a really good chance of finding an electron pair as they don't remain still but move around the charge cloud
Answer: As charge clouds
Answer: In dative covalent, also known as co-ordinate bonding, one atom provides both of the shared electron in the bond.
Answer: Due to its tetrahedral
Answer: All the outer electrons are held in localized bonds so cannot move and carry charge
Answer: Vibrations can travel easily through the stiff lattice
Answer: There are strong covalent bonds between atoms that require a lot of energy to overcome
Very high melting point
Extremely hard
Good thermal conductor
Can't conduct electricity
Insoluble
Can be cut to form gemstones and refract light
Answer: Tetrahedral
Answer: The covalent bonds in the sheets are too strong to break
Answer: The strong covalent bonds in the sheets require a lot of energy to overcome
Answer: The layers of hexagons are quite far apart compared to the length of the covalent bonds
Answer: It contains delocalised electrons which aren't attached to any particular carbon atom so are free to move and carry charge
Answer: The weak bonds between sheets of graphite are easily broken allowing them to slide over each other
Answer: Bc each carbon atom can form 4 strong covalent bonds
Answer: Huge networks of atoms held together by strong covalent bonds
Answer: covalent bonds
Answer: Water molecules are polar so the partially charged poles attract the oppositely charged ions away from each other and the lattice causing it to dissolve
Answer: Giant ionic lattices are held together by strong forces of electrostatic attraction which require a lot of energy to overcome
The ions in a liquid are free to move and carry charge
In a solid the ions are fixed in position by strong forces of electrostatic attraction
Answer: Giant lattices of ions
Answer: 0